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The heat capacity ratio of an ideal gas is 1.38. What are its Cv and Cp values?
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- What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?What is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
- What is the ∆rxnG° (in KJ/mole) for a mole of an ideal gas as pressure changes from 0.1 Pa to 1×10^5 Pa?Calculate ΔStotal (for the system) when the state of 0.8 mol diatomic perfect gas molecules, for which Cp,m = 7/2R, is changed from 25°C and 1.50 atm to 135°C and 7.00 atm.Express answer in J/K.What is the heat capacity at constant colume n mole monatomic gas a. 3/2nH b. 5/2nR c. 7/2nR d. 9/2nR
- Two iron bolts of equal mass—one at 100.°C, the other at 55°C—are placed in an insulated container. Assuming the heatcapacity of the container is negligible, what is the final tempera-ture inside the container (c of iron =0.450 J/g.K)?Calculate DH and DStot when two copper blocks, each of mass 10.0 kg, one at 100°C and the other at 0°C, are placed in contact in an isolated container. The specific heat capacity of copper is 0.385 J K−1 g−1 and may be assumed constant over the temperature range involved.1 mol of an ideal gas at 25 ° C and 10 atmospheres (Cp = 3.5 R), adiabatically and reversibly 5 What will be the final volume and temperature when it expands into the atmosphere?
- Cp− ̄Cv=T ̄V β^2/κ reduces to ̄CP− ̄CV=R for an ideal gas.A fuel has the following volumetric analysis: CH4 = 68% C2H6 = 32% Assume complete combustion with 15% excess aur at 101.325 kPa and 27 degrees dry bulb temperature. What is the total moles in the products of combustion?12) Between 0 °C and 100 °C, the heat capacity of Hg(l) is given by: Cp,m (Hg, l) [units: J mol-1 K-1] = 30.093 – 4.944 x 10-3T Calculate ΔH and ΔS if the temperature of 1.75 moles of Hg(l) is raised from 0.00 °C to 100.00 °C at constant P.