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# Heat capacity Water J / (mol K)

Water in liquid form having a molar heat capacity H2O: 75.338 J/K*mol (25°C, 101.325 kPa) Read more. T [K] P [kPa] Molar Heat Capacity (cP) [J/(mol*K)] State Reference; 271.56: 49033.000: 72.79: Liquid: 1: 272.21: 88260.000: 71.09: Liquid: 1: 272.25: 68647.000: 71.83: Liquid: 1: 272.71: 68647.000: 71.84: Liquid: 1: 272.75: 88260.000: 71.10: Liquid: 1: 272.90: 49033.000: 72.82: Liquid: 1: 273.00: 49033.000: 72.77: Liquid: 1: 273.22: 29420.000: 74.05: Liquid: 1: 273.22: 68647.000: 71.91: Liquid: 1: 273.22: 88260.000: 71.11: Liquid: 1: 273.24: 49033.00

### Heat capacity water j/mol k — the molar heat capacity of

The molar heat capacity of liquid water is 75.348 J/mol K. It is calculated as the product of the specific heat capacity of liquid water and the molar mass of water. The specific heat capacity of liquid water is 4.186 J/gm K 69.95 J/(mol K) Heat capacity, c p: 75.97 J/(mol K) and 4.2176 J/(g·K) at 0 °C 75.42 J/(mol K) and 4.1921 J/(g·K) at 10 °C 75.33 J/(mol K) and 4.1818 J/(g·K) at 20 °C 75.28 J/(mol K) and 4.1814 J/(g·K) at 25 °C 75.26 J/(mol K) and 4.1784 J/(g·K) at 30 °C 75.26 J/(mol K) and 4.1785 J/(g·K) at 40 °C 75.30 J/(mol K) and 4.1806 J/(g·K) at 50 °C 75.37 J/(mol K) and 4.1843 J/(g·K) at 60 ° Online Water Specific Heat Calculator. The calculator below can be used to calculate the liquid water specific heat at constant volume or constant pressure and given temperatures. The output specific heat is given as kJ/ (kmol*K), kJ/ (kg*K), kWh/ (kg*K), kcal/ (kg K), Btu (IT)/ (mol*°R) and Btu (IT)/ (lb m *°R) Note Note that the especially high molar values, as for paraffin, gasoline, water and ammonia, result.

### Molar Heat Capacity (cP) of Water from Dortmund Data Ban

The molar heat capacity of water, CP, is 75.2 J mol⋅K 75.2 J mol ⋅ K. How much heat is required to raise the temperature of 36 grams of water from 300 to 310 K? We are given the molar heat capacity of water, so we need to convert the given mass of water to moles The heat capacity of liquid water is 75.6J/K - mol, while the enthalpy of fusion of ice is 6.0kJ/mol. What is the smallest number of ice cubes at 0^oC, each containing 9.0g of water, needed to cool 500g of liquid water from 20^oC to 0^oC ? 11t heat transfer. Heat capacity of The Elements Table Chart. Heat Transfer Thermodynamics. Heat capacity of The Elements at 25° C. This table gives the specific heat capacity (cp) in J/g K and the molar heat capacity (Cp) in J/mol K at a temperature of 25°C and a pressure of 100 kPa (1 bar or 0.987 standard atmospheres) for all The elements for which reliable data are available The heat capacity of water is 4.18 J g -1 K -1. Calculate the energy, in kJ, required to boil 1.2 L of water, starting at 25 °C. Boiling water from 25 °C requires raising its temperature by another 75 °C, so ΔT = 75 K (100-75). The mass of water in g, is calculated by multiplying volume by density

The specific heat - C P and C V - will vary with temperature. When calculating mass and volume flow of a substance in heated or cooled systems with high accuracy - the specific heat (= heat capacity) should be corrected according values in the table below. Specific heat of Water Vapor - H 2 O- at temperatures ranging 175 - 6000 K calorie, the specific heat of water is 4.184 J/g-K. The ease with which a substance gains or loses heat can also be described in terms of its molar heat capacity, which is the heat required to raise the temperatur Mathematically, it is the heat capacity of a substance divided by the number of moles and is expressed as: Here, c m is molar heat capacity (J/K.mol), C is heat capacity (J/K), and n is the number of moles (mol)

Click here������to get an answer to your question ️ The molar heat capacity of water at constant pressure, Cp is 75 J K^-1 mol^-1 . When 10 KJ of heat is supplied to 1 kg water which is free to expand, the increase in temperature of water is Calculate the amount of heat (in Joules) required to change the temperature of 1 Liter of water (1 L = 1 Kg) from 20˚C to 37˚C. The specific heat capacity (C) of water is 4.184 J/g˚C (or J/g·K — as long we work with Celsius degrees or Kelvins, the ΔT will be the same because the size of the two are the same Heat capacity, or thermal capacity, is the measurable physical quantity of heat energy required to change the temperature of an object by a given amount. Its SI unit is joule per Kelvin. Heat capacity is an extensive property of matter, meaning it is proportional to the size of the system

### What Is the Molar Heat Capacity of Liquid Water

1. The specific heat capacity of water is 4.2 J/g·°С. Thus, the heat capacity of a 50 g espresso shot is about 210 J/°С
2. Molar heat capacity of water is 75.3 J mol^-1 K^-1 - Sarthaks eConnect | Largest Online Education Community Calculate the amount of heat necessary to raise 180 g of water from 25°C to 100°C. Molar heat capacity of water is 75.3 J mol^-1 K^-1 ← Prev Question Next Question �
3. The molar heat capacity (Cp) is the amount of energy needed to increase the temperature of 1 mol of a substance by 1°C; the units of Cp are thus J/ (mol•°C). The subscript p indicates that the value was measured at constant pressure
4. um: 0.900: 0.215: 24.3: Bismuth: 0.123: 0.0294: 25.7: Copper: 0.386: 0.0923: 24.5: Brass: 0.
5. Water has a molar specific heat capacity of 75.32 J/mol·K. Copper has a molar specific heat capacity of 24.78 J/mol·K. Molar Heat Capacity Versus Specific Heat Capacity While molar heat capacity reflects the heat capacity per mole, the related term specific heat capacity is the heat capacity per unit mass
6. joule per kilogram kelvin: J kg-1 K-1: joule per gram kelvin: J g-1 K-1: joule per gram degree Celsius: J g-1 o C-1: calorie IT per gram degree Celsius: cal IT g-1 o C-1: British thermal unit IT per pound degree Fahrenheit: Btu IT lb-1 o F-1: British thermal unit IT per pound degree Rankine: Btu IT lb-1 o R-1: calorie th per gram degree Celsius: cal th g-1 o C-1: British thermal unit th per.
7. Free online specific heat capacity converter - converts between 20 units of specific heat capacity, including joule/kilogram/K [J/(kg*K)], joule/kilogram/°C [J/(kg*°C)], joule/gram/°C [J/(g*°C)], kilojoule/kilogram/K, etc. Also, explore many other unit converters or learn more about specific heat capacity unit conversions

The heat of combustion of CH4 is 890.4 kJ>mol, and the heat capacity of H2O is 75.2 J>mol # K. Find the volume of methane measured at 298 K and 1.00 atm required to convert 1.00 L of water at 298 K to water vapor at 373 K The molar heat capacity of ice is 37 J mol-1 K-1 and the molar heat capacity of liquid water is 76 J mol-1 K-1 . What can be concluded about the relative magnitudes of the heat of fusion of ice at 263 K (∆H263) compared to the heat of fusion of ice at 273 K (∆H273) /(J K−1 mol−1)* 29 136.1 24.44 111.46 37 75.29 33.58 * Molar heat capacities are given only for air and well-defined pure substances; see also the Data section. The text's website contains links to online databases of heat capacities. 40 Molar constant-pressure heat capacity, Cp,m/(J K-1 mol-1) H Temperature, T Cp,m Heat capacity.

1. The molar heat capacity of water, CP, is 75.2 $\frac{J}{mol\bullet K}$. How much heat is required to raise the temperature of 36 grams of water from 300 to 310 K? We are given the molar heat capacity of water, so we need to convert the given mass of water to moles
2. Specific Heat Table. Summary. The specific heat of water is 4182 J/kg°C, which is a high specific heat capacity and is sometimes taken as 4,200 J/kg °C for ease in calculations. Specific heat capacity is the defined as the amount of heat per unit required to raise the temperature by one degree Celsius
3. 25200J E = mcDeltatheta where c is specific heat capacity in J//g//K (specific heat capacity: the amount of energy needed to raise the temperature of 1g of a substance by 1K) and Deltatheta is the change in temperature. here, Deltatheta = 50^@C - 20^@C = 30^@C. E = 200g * 4.2 J//g//K * 30K = 25200
4. Assume that the heat capacity of water is (4.184 J/(K-g))(18 g/mol) = 75.3 J/(K-mol) and that the heat capacity of the calorimeter is negligible. I was wondering if the following general methodology of my attempt was correct. In attempting to solve this, I first found that the equilibrium temperature was (273+373)/2 = 323 K

Their SI units are J/kg K or J/mol K. Two specific heats are defined for gases, one for constant volume (c v) and one for constant pressure (c p). According to the first law of thermodynamics, for constant volume process with a monatomic ideal gas the molar specific heat will be: C v = 3/2R = 12.5 J/mol K. because. U = 3/2nR Heat Capacity of Liquid and Solid Polymers at 298 K (1); Polymer / Heat Capacity (J/mol-K): C p,solid: C p,liquid: Poly(acrylonitrile), PAN: 69.3-Poly(Bisphenol A carbonate), P

The symbol for the Universal Gas Constant is Ru= 8.314 J/mol.K (0.0831 bar dm3 mol-1 K-1).The Specific-Heat Capacity, C, is defined as the amount of heat required to raise the temperature by 1K per mole or per kg.The Specific Heat Capacity is measured and reported at constant pressure (Cp) or constant volume (Cv) conditions.For monoatomic gases Cp=2.5Ru J/mol.K and Cv=1.5Ru J/mol.K repectively NH3 (molecular weight 17) has even a slightly higher *specific* heat capacity than water at similar conditions, again mainly because of the low molar mass. So there is nothing really peculiar about the specific heat capacity of water Answer to: The constant pressure molar heat capacities of ice and water are 37.7 J mol^{-1} K^{-1} and 75.3 J mol^{-1} K^{-1} respectively. The..

The heat capacity of liquid water is 75 6 J / mol K, while the enthalphy of fusion of ice is 6 0 KJ/ mol What is the smallest number of ice cubes at 0 C , each conatining 9 0 g of water , needed to cool 500g - Chemistry - Thermodynamic Specific heat of Silver is 0.235 J/g K. Latent Heat of Fusion of Silver is 11.3 kJ/mol. Latent Heat of Vaporization of Silver is 250.58 kJ/mol. Specific Heat. Specific heat, or specific heat capacity, is a property related to internal energy that is very important in thermodynamics Sources. PAff: Proton affinity (kJ/mol). BasG: Gas basicity (kJ/mol). ΔcH°solid: Standard solid enthalpy of combustion (kJ/mol). Cp,gas: Ideal gas heat capacity (J/mol×K). Cp,solid: Solid phase heat capacity (J/mol×K). SProt: Protonation entropy at 298K (J/mol×K) The heat capacity of liquid water is 75.3 J/mol ∙ K. The conversion of 50.0 g of ice at 0.00 °C to liquid water at 0.00°C requires _____ kJ of heat. Question 21 options: 6.01 16.7 75.3 17.2 Insufficient data are given. This problem has been solved! See the answer See the answer See. Given that the heat of fusion of water is -6.02 kJ>mol, the heat capacity of H2O (l) is 75.2 J>mol # K, and the heat capacity of H2O (s) is 37.7 J>mol # K, calculate the heat of fusion of water at -10 u001fC

### Water (data page) - Wikipedi

• The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol K. The conversion of 20.0 g of ice at 0.0 °C to liquid water at 30.0°C requires kJ of heat. 17.2 O 16.7 O 9.19 O Insufficient data are given. 18.
• ∆fH° Standard molar enthalpy (heat) of formation at 298.15 K in kJ/mol ∆fG° Standard molar Gibbs energy of formation at 298.15 K in kJ/mol S° Standard molar entropy at 298.15 K in J/mol K Cp Molar heat capacity at constant pressure at 298.15 K in J/mol K The standard state pressure is 100 kPa (1 bar)
• For instance, S° for liquid water is 70.0 J/(mol·K), whereas S° for water vapor is 188.8 J/(mol·K). Likewise, S° is 260.7 J/(mol·K) for gaseous I 2 and 116.1 J/(mol·K) for solid I 2. This order makes qualitative sense based on the kinds and extents of motion available to atoms and molecules in the three phases
• When 0.46 g of ethanol is burned under a water-filled calorimeter, the temperature of 500 g of water is raised by 3.0 K. (Molar mass of ethanol = 46 g mol -1; specific heat capacity of water = 4.18 J g -1 K -1; q = mc ∆ T.
• 29. For the vaporization of water at 1.00 atm, H = 43.54 kJ/mol at 298 K and H = 40.68 kJ/mol at 373 K The constant-pressure heat capacity of liquid water is 75.3 J/mol • K. Calculate the constant-pressure heat capacity for H 2 O(g). A) 20.8 J/mol•K B) 37.2 J/mol•K C) 2790 J/mol•K D) 75.3 J/mol•K E) none of these Use the following to answer questions 30-32: Two samples of a monatomic.
• The specific heat capacity of porcelain is around 0.8 J/g·°С. A typical porcelain espresso cup weighs about 60 grams, so it has a heat capacity of about 50 J/°С. The specific heat capacity of water is 4.2 J/g·°С. Thus, the heat capacity of a 50 g espresso shot is about 210 J/°С
• Specific heat of Nitrogen is 1.04 J/g K. Latent Heat of Fusion of Nitrogen is 0.3604 kJ/mol. Latent Heat of Vaporization of Nitrogen is 2.7928 kJ/mol. Specific Heat. Specific heat, or specific heat capacity, is a property related to internal energy that is very important in thermodynamics 1.6B Heat Capacity. The heat capacity of a substance is defined as the amount of heat necessary to increase the temperature by 1 degree. It can be expressed for 1 g, 1 lb, 1 g mol, 1 kg mol, or 1 lb mol of the substance. For example, a heat capacity is expressed in SI units as J/kg mol · K; in other units as cal/g · °C, cal/g mol · °C, kcal/kg mol · °C, Btu/lb m · °F, or btu/lb mol. Calculate the heat of vaporization of water at 298 K given its value at 393 K is 2.26 × 10 6 J/kg. The specific heat of water is 4.184 × 10 3 J/K/kg and its heat capacity at constant pressure is 33.47 J/K/mol. Assume that the heat capacity..

J K 1 mol 1 S°(J K-1mol-1) Gl ucose -1273.1 219.2 209.2 Lactic acid -673.6 127.6 192.1 Calculate the entropy of the system, the surroundings, and the universe at T = 310. K. Assume the heat capacities are constant between T = 298 K and T = 330. K. The standard entropy and enthalpy and heat capacity for this reaction are: note: here C P. The heat capacity of liquid water is 4.18 J/g C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67 C into. 37,821 results, page 15 Example $$\PageIndex{2}$$: Heat Capacity of a Calorimeter. In determining the heat capacity of a calorimeter, a student mixes 100.0 g of water at 57.0 °C with 100.0 g of water, already in the calorimeter, at 24.2°C. (yhe specific heat of water is 4.184 J g-1 K-1)

30) The molar heat capacity of an unknown substance is 92.1 J/mol-K. If the unknown has a molar mass of 118 g/mol, what is the specific heat (J/g-K) of this substance? A) 1.28 B) -92.1 C) 1.09 × 104 D) 0.781 E) 92. Specific heat capacity Unit Converter Online. 15. kilogram-force meter/kilogram/K

### Water - Specific Heat - Engineering ToolBo

In this case, the heat is added at constant pressure, and we write. (3.6.4) d Q = C p n d T, where C p is the molar heat capacity at constant pressure of the gas. Furthermore, since the ideal gas expands against a constant pressure, (3.6.5) d ( p V) = d ( R n T) becomes. (3.6.6) p d V = R n d T. Finally, inserting the expressions for dQ and pdV. What is the specific heat capacity of water? The specific heat of water is 1 calorie/gram °C = 4.186 joule/gram °C which is higher than any other common substance. As a result, water plays a very important role in temperature regulation. The specific heat per gram for water is much higher than that for a metal, as described in the water-metal example One calorie= 4.184 joules; 1 joule= 1 kg (m)2(s)-2 = 0.239005736 calorie. The specific heat capacity of water vapour at room temperature is also higher than most other materials. For water vapour at room temperature and pressure, the value of specific heat capacity (Cp) is approximately 1.9 J/g°C. As with most liquids, the temperature of water. The molar heat capacity of Al is 24 J/(mol.K), and the heat of fusion of Al is 10.7 kJ/mol. To raise the temperature from 298 K to 933 K: 24 J x 1.00 mol x 635 K = 15,000 J = 15 kJ mol K It takes 10.7 kJ to melt the Al at 933 K. 15 kJ + 10.7 kJ = 26 kJ I point is earned for calculating the amount of heat needed to raise the temperature to 933 K. Specific heat is defined by the amount of heat needed to raise the temperature of 1 gram of a substance 1 degree Celsius (°C).Water has a high specific heat capacity which we'll refer to as simply heat capacity, meaning it takes more energy to increase the temperature of water compared to other substances

### Table of specific heat capacities - Wikipedi

Molar heat capacities. If the molar heat capacities (the heat required to raise the temperature of one mole of a substance by 1 K) of metals are considered, then it is found that they are all approximately the same and equal to about 25 J mol-1 K-1, a fact first noticed by Dulong and Petit in 1819 (Specific heat capacity of water = 4.2 J K 1 g 1) (4 marks) 4. The experimental value obtained by the student is considerably lower than the theoretical value calculated. Suggest one reason for this (other than experimental error). 26891 J = mass of water × 4.2 J K 1 mol 1 1. Answer to: The heat of combustion of CH_4 is 890.4 kJ/ mol and the heat capacity of H_2O is 75.2 J/ mol . K. Find the volume of methane measured at.. Answer: 3 ������������������ question Given that the heat of fusion of water is +6.02 kJ/molkJ/mol, that the heat capacity of H2O(l)H2O(l) is 75.2 J/mol⋅KJ/mol⋅K and that the heat capacity of H2O(s)H2O(s) is 37.7 J/mol⋅KJ/mol⋅K, calculate the heat - the answers to estudyassistant.co

### Heat - Purdue Universit

Page 1 of 1 Chemistry 121 - Summer 2008 - Worksheet #9 1. The molar specific heat capacity of mercury is 28.1 J/mol K. What is the specific heat capacity of this metal in J/g K How much heat is needed to raise the temperature of 75.2 mol of water (heat capacity of 4.184 J/g-1-K-1) from 12.5°C to 80.0°C? Online Text . 6 . A sample of aluminum absorbed 9.86 J of heat, and its temperature increased from 23.2°C to 30.5°C. What was the mass of the aluminum sample? (The specific heat of aluminum is 0.90 J/g-K. Calculate the heat capacity of the calorimeter in J/K. Solution: The hot water loses heat, the cold water gains heat, and the calorimter itself gains heat, so this is essentially a thermal balance problem. Conservation of energy requires that . q hot + q cold + q cal = 0. We can evaluate the first two terms from the observed temperature changes.

### Molar Heat Capacity: Definition, Formula, Equation

Heat Capacity 4. Atkins - Ex. 2.4(b) (heat expansion) A sample consisting of 2.00 mol of perfect gas molecules, for which CV,m = 5/2R, initially at P1 = 111 kPa and T1 = 277 K, is heated reversibly to 356 K at constant volume The molar heat capacity is the heat capacity per mole of material. For most materials the molar heat capacity is 25 J/mol K. In order to determine the heat capacity of a substance we not only need to know how much heat is added, but also the conditions under which the heat transfer took place Th e heat capacity of air is much smaller than that of water, and relatively modest amounts of heat are needed to change its temperature. Th is is one of the reasons why desert regions, although very hot during the day, are bitterly cold at night. Th e heat capacity of air at room temperature and pressure is approximately 21 J K−1 mol−1 But unfortunately, there is evil adblock script and he ate me : (. Most popular convertion pairs of heat capacity. Kilojoule/Kilogram K → BTU/Pound °F. Joule/Kilogram K → BTU/Pound °F. Joule/Gram °C → BTU/Pound °F. Kilojoule/Kilogram °C → BTU/Pound °F. Calorie/Gram °C → BTU/Pound °F

Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -15 ∘C In chemistry, however, they make use of molar heat capacity Cmol, which just adds the mol variable in the equation Cmol = J / mol . K. On the other hand, specific heat sounds similar to heat capacity in terms of definition, but the former refers to the needed heat to adjust the temperature of a single unit of a substance's mass by one degree Calculate the heat and work requirements and ΔU and ΔH of the air for each path. The following heat capacities for air may be assumed independent of temperature: C V = 20.78 and C P =29.10 J mol-1 K-1 Assume also for air that PV/T is a constant, regardless of the changes it undergoes. At 298.15K and 1 bar the molar volume of air is 0.02479 m3. Heat Capacity for 100g Ice = 203 J/C; Heat Capacity for 1g Ice = 2.03 J/C per gram; If you are confused, think of it this way -- it takes 2.03 Joules to raise every single gram of ice one degree. So, if we have 100 grams of ice we need 100 times as many Joules to heat it all The water at the bottom of the Niagara Falls, which are 50 m high, should be warmer than that at the top. Explain why it is and calculate the temperature rise. The heat capacity of 1 mol water (which weighs 0.018 kg) is 80 J/K. The acceleration due to gravity is 9.8 m/s 2

Specific Heat Capacity Examples. Water has a specific heat capacity of 4.18 J (or 1 calorie/gram °C). This is a much higher value than that of most other substances, which makes water exceptionally good at regulating temperature. In contrast, copper has a specific heat capacity of 0.39 J The molar heat capacity of the gas at constant volume is 30 J mol‒1 K‒1 (assumed to be independent of temperature); universal gas constant, R is 8.314 J mol‒1K‒1; ratio of molar heat capacities is 1.277. The temperature (in K, rounded off to the first decimal place) of the gas at the final state in the irreversible compression case is____ Q. The combustion of titanium with oxygen produces titanium dioxide. When 2.060 g of titanium is combusted in a bomb calorimete, the temperature of the calorimeter increases from 25.00 ° C \degree C ° C to 91.60 ° C \degree C ° C .In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K Joule/Gram °C : The joule per gram per degree Celsius is a metric unit of specific heat capacity. Its symbol is J/g•°C. Kilojoule/Kilogram K : The kilojoule per kilogram per kelvin is a unit of specific heat capacity, which is a decimal multiple of the SI derived unit of joule per kilogram per kelvin. Its symbol is kJ/kg•K. Heat Capacity Conversion Calculato    The heat of combustion of CH 4 is 890.4 kJ/mol and the heat capacity of H 2 O is 75.2 J/molK. Find the volume of methane measured at 298 K and 1.26 atm required to convert 1.01 L of water at 298 K to water vapor at 373 K Question from Chemical Thermodynamics,jeemain,chemistry,class11,unit6,chemical-thermodynamics,eas 36.A 22.4-g piece of aluminum (which has a molar heat capacity of 24.03 J/mol°C) is heated to 84.8°C and dropped into a calorimeter containing water (the specific heat capacity of water is 4.18 J/g°C) initially at 22.8°C. The final temperature of the water is 27.0°C. Calculate the mass of water in the calorimeter We define the molar heat capacity at constant volume C V as. C V = 1 n Q Δ T ⏟ with constant V. This is often expressed in the form. Q = n C V Δ T. If the volume does not change, there is no overall displacement, so no work is done, and the only change in internal energy is due to the heat flow Δ E i n t = Q Evaluation of heat capacities (also known as specific heats). Cp and CV have units of energy per amount per temperature interval, where the amount of material may be measured in molar or mass units (e.g. units of heat capacity could be J/(kg oC), J/(mol oC), etc). Table B.2 provides polynomial expressions for heat capacities Cp Cp = a + bT. How much heat would be required to convert 234.3 g of solid benzene, C6H6(s), at 5.5 °C into benzene vapor, C6H6(g), at 100.0 °C? Benzene has the following molar heat capacities: C6H6(l) = 136 J/mol °C, and C6H6(g) = 81.6 J/mol °C The molar heat of fusion for benzene is 9.92 kJ/mol and the molar heat of vaporization for benzene is 30.8 kJ/mol