A sample of 1.3 mol of CO2 (g) is placed in a 5.0 L rigid container at an initial temperature is 300 K. When 6.98 kJ of heat is added to the system (at constant volume), the temperature rises to 353 K. Calculate q, w, ∆U, ∆H, and CV.
The molar heat capacity of O2(g) at constant pressure, is 31.2 J/(K mol) around room temperature. 2.5 mol of O2(g) is heated at constant pressure from 265 K to 310 K. Calculate q, w, ∆H, and ∆U.
A sample of 1.3 mol of CO2 (g) is placed in a 5.0 L rigid container...
A sample of 5.0 mol CO2(g) is originally confined in 15 dm3 at 280 K and then undergoes adiabatic expansion against a constant pressure of 78.5 kPa until the volume has increased by a factor of 4.0. Calculate q, w, delta T, and delta U, and delta H. (The final pressure of the gas is not necessarily 78.5 kPa.) If the enthalpy you calculate does not equal -4.5 kJ and the temperature change - 24 K, you made a mistake.
4. An ideal gas of 5.0 mol CO2 is originally confined in 15 L at 300 K. Assume it undergoes isothermal expansion against a constant pressure of 1.0 atm until equilibrium is reached. Assume the heat capacity of CO2 at constant pressure, Cp.m is 37.11 J/mol K. Calculate the final volume, q, w,aU, and △H for the process. (15%) 5. Calculate the minimum work needed to freeze 250 g of water originally at 0°C standing in a room at 20°C....
1. A 0.050-mol sample of NO2 was placed in a 10.0-L container and heated to 750 K. 2NO2(g) → 2NO(g) + O2(g) The total pressure of the equilibrium mixture as a result of the decomposition was 0.414 bar. What is the value of K at this temperature? 2. The equilibrium constant (Kw) for the equation H20(1) - H+(aq) + OH-(aq) was measured at several temperatures. Determine ArH (298K) for the reaction using the following data: T('C) 10 20 30 40...
At a certain temperature, 0.700 mol of SOs is placed in a 2.00-L container. 2502(g) + O2 At equilibrium, 0.140 mol of O2 is present. Calculate K. Number
A 10 L container is filled with 0.10 mol of H2(g)and heated to 2800 K causing some of the H2(g) to decompose into H(g). The pressure is found to be 3.0 atm. Find the partial pressure of the H(g) that forms from H2 at this temperature. (Assume two significant figures for the temperature.)
At a particular temperature, 12.0 mol of SO_3 is placed into a 3.0-L rigid container, and the SO_3 dissociates by the reaction| 2SO_3(g) 2SO_2(g) + O_2(g) At equilibrium, 3.0 mol of SO_2 is present. Calculate K_c for this reaction. 1.5 0.11 0.72 0.056 0.17 0.0035
A sample of nitrogen gas contains 5.0 mol in a volume of 3.5 L. Calculate the new volume of the container if the pressure and temperature are kept constant but the number of moles of nitrogen is changed to 1.4 mol
A sample of 18 g of oxygen gas (O2) is confined in a container at 200 kPa and 273 K. The gas is allowed to expand adiabatically and reversibly to 100 kPa. Calculate the final temperature of the gas. The molar heat capacity at constant pressure (CP,m) of O2 is 29.355 J mol-1 K-1
At a certain temperature, 0.680 mol SO2 is placed in a 4.50 L container. 2503(g) = 2502(8) + O2(8) At equilibrium, 0.110 mol O, is present. Calculate Kc. K=
At a certain temperature, 0.740 mol SO, is placed in a 5.00 L container. 2 SO3(g) = 2502(g) + O2(g) At equilibrium, 0.180 mol 0, is present. Calculate K. Ko