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6. Use the following data at 298.15 K to complete this problem: ( mol) 8.95 241.841...
Part A Use the following data at 298.15 K to complete this problem: ΔH∘R(kJ⋅mol−1) 1/2H2(g)+1/2O2(g)→OH(g) 38.95...
Part A Use the following data at 298.15 K to complete this problem: ΔH∘R(kJ⋅mol−1) 1/2H2(g)+1/2O2(g)→OH(g) 38.95 H2(g)+1/2O2(g)→H2O(g) -241.841 H2(g)→2H(g) 435.994 O2(g)→2O(g) 498.34 Assuming ideal gas behavior, calculate ΔH∘R and for the following reaction: OH(g)→H(g)+O(g) Express your answer to five significant figures and include the appropriate units. Part B Assuming ideal gas behavior, calculate ΔU∘R and for the following reaction: OH(g)→H(g)+O(g) Express your answer to five significant figures and include the appropriate units. Part C Assuming ideal gas behavior, calculate ΔH∘R...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 14.96 mm Hg. 2N2(g) + O2(g)2N2O(g) G =_____ kJ/mol
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 18.65 mm Hg. 2NO(g) + O2(g)2NO2(g) G = ____kJ/mol
a.) Calculate the equilibrium constant for the following reaction at 298.15 K from cell potential data....
a.) Calculate the equilibrium constant for the following reaction at 298.15 K from cell potential data. Express the answer as lnK. Sn4+ + 2Fe2+ ----> Sn2+ + 2Fe3+ b.) Calculate the standard Gibbs free energy change in kJ/mol at 298.15 K for the following reaction from cell potential data: 3Sn4+ + 2Cr ----> 3Sn2+ + 2Cr3+
You have a 3.00-L container filled with N₂ (MM = 28.02 g/mol) at 298.15 K and...
You have a 3.00-L container filled with N₂ (MM = 28.02 g/mol) at 298.15 K and 1.75 atm pressure connected to a 2.00-L container filled with Ar (MM = 39.95 g/mol) at 298.15 K and 2.15 atm pressure. A stopcock connecting the containers is opened and the gases are allowed to equilibrate between the two containers. What is the density of the final gas mixture? Assume ideal behavior. (Use R = 0.08206 L.atm/mol.K) (HINT: What is the total mass, m,...
Calculate the free energy change under nonstandard state conditions. Close Problem Use standard thermodynamic data (in...
Calculate the free energy change under nonstandard state conditions. Close Problem Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 13.54 mm Hg. CO(g) + Cl2(g)COCl2(g) G = kJ/mol
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
Need help with 4.6 temperatui water is 1.60 K. Calculate Δ1) and an Calculate Δ H2...
Need help with 4.6
temperatui water is 1.60 K. Calculate Δ1) and an Calculate Δ H2 for NO(g) at 975 K, assuming that the als P4.4 heat capacities of reactants and products are constant over the tie temperature interval at their values at 298.15 K. P4.5 The total surface area of the earth covered by ocean is cu 335 × 108 km2. Carbon is fixed in the oceans via photosyn- thesis performed by marine plants according to the reaction 6...
Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction....
Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. HCl(g) + NH3(g)--->NH4Cl(s) K =
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
Need help with 4.6
temperatui water is 1.60 K. Calculate Δ1) and an Calculate Δ H2 for NO(g) at 975 K, assuming that the als P4.4 heat capacities of reactants and products are constant over the tie temperature interval at their values at 298.15 K. P4.5 The total surface area of the earth covered by ocean is cu 335 × 108 km2. Carbon is fixed in the oceans via photosyn- thesis performed by marine plants according to the reaction 6...
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