Data: Standard molar enthalpy of melting of ice at 273 K: AmeltH (H₂O, 273 K) = 6.02 kJ mol-¹ Average values of the specific heat capacities at constant pressure P° = 1 bar: Cp (H₂O; s) = 37.6 J K-¹ mol-¹ Cp (H₂O; 1) = 75.2 J K-¹ mol-¹ Calculate AfreezS°(H₂O; 273 K), the standard molar entropy of freezing of water at 273 K.

Data: Standard molar enthalpy of melting of ice at 273 K: AmeltH (H₂O, 273 K) = 6.02 kJ mol-¹ Average values of the specific heat capacities at constant pressure P° = 1 bar: Cp (H₂O; s) = 37.6 J K-¹ mol-¹ Cp (H₂O; 1) = 75.2 J K-¹ mol-¹ Calculate AfreezS°(H₂O; 273 K), the standard molar entropy of freezing of water at 273 K.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Similar questions

Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Trouton's rule states that the molar enthalpy of Chemical AHvap Boiling AHfus Compound vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion-ion attractions is given by formula (kJ-mol-1) point (K) (kJ-mol¬1) chloromethane CH;CI 21.40 249.06 6.43 AH vap (85 J. K-1. mol-') To H,0 water 40.65 373.15 6.01 where T, is the normal boiling point of the liquid hydrogen H,S 18.67 213.60 18.67 in kelvins. sulfide Apply Trouton's rule to estimate the value of AHvap for these compounds. chloromethane: AHvap kJ/mol
Formation of carbon dioxide Data: Standard molar enthalpy of formation of CO2 (g) at 300 K: A¢H°(CO2, g; 300 K) = - 393.09 kJ mol-! Molar heat capacities at constant pressure (Cp): C (graphite) 20.27 J mol·' K-' O2 (g) 36.57 J mol·' K-' CO2 (g) 31.56 J mol·' K-' Let's consider the reaction of formation of CO2 (g) and its associated molar enthalpy of formation at 1200 K. - This reaction can be considered as another particular case of reaction. Which one? Calculate the standard molar enthalpy of formation of CO2 (g) at 1200 K.
4.00 g NaOH(s) (39.996 g mol–1) dissolves in 100.0 g of water in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The density of the solution is 1.00 g cm–3. The heat of dissolution is –44.51 kJ mol–1. The specific heat of the solution is 4.184 J g–1 °C–1. The specific heat of the calorimeter is 100 J °C–1. What is the final temperature of the solution? 30.23°C 25.94°C 28.32°C What is the energy lost to the calorimeter? 579 J 832 J 721 J
Determine the change in standard enthalpy, in units of kJ mol-1, for the following reaction: C(s, graphite) + 2 H2(g) + ½ O2(g) CH3OH() A,H = ? using the following reaction data: C(s, graphite) + O2(g) CO2(g) ArH = -393.5 kJ mol-1 H2(g) + ½ O2(g) H20() A,H = -285.8 kJ mol-1 2 CH3OH() + 3 O2(g) → 2 CO2(g) + 4 H20() A,H = -1452.8 kJ mol-1
Water freezing Data: Standard molar enthalpy of melting of ice at 273 K: AmeltH°(H2O, 273 K) = 6.02 kJ mol- %3D Average values of the specific heat capacities at constant pressure P° = 1 bar: Cp (H2O; s) = 37.6 J K-' mol-! Cp (H2O; 1) = 75.2 J K-' mol! Calculate the standard molar enthalpy of freezing of supercooled water at 268 K: AfreezH°(H2O; 268 K). Water is supercooled water when it is liquid at T < Tmelt-
The atomic heat capacity of solid Mo is given by the equation 0.503 x 105 Cp = 5.69 + 1.88 x 10-3 T – T² Find the change in entropy (in eu) which accompanies the heating of one mole of Mo from o C to its melting point, 2620°C. (Entropy unit, (eu) equal to i cal K-¹). Cp expression gives heat capacity in units of cal/mol.
13. (a) How much heat wiH be evolved or absorbed in the solution of 2 moles of H,SO,(1) in a very large volume of water at 25°C? (b) What will be the dif- ferential heats of solution of the acid and the water under these conditions?
Find A,U for the combustion of methanol (CH3 OH) to carbon dioxide and liquid water from the following data: The heat capacity of the bomb calorimeter is 34.65 kJ K 1 The combustion of 1.771 g of methanol raises the temperature of the calorimeter from 294.370 K to 295.528 K. The molar mass of methanol is 32.04 g mol1. Enter your answer using four significant figures. ? A;U = kJ mol1