47. Solution to Chemistry Problem

For the chemical reaction involving gaseous substances given in Table 1, perform the following thermodynamic calculations:
1. Calculate the heat of reaction at standard temperature at constant pressure ΔH0298 and constant volume ΔU0298;
2. Calculate the heat of reaction at temperatures T1, T2, T3 using the temperature dependences of heat capacities. Plot a graph of the heat of reaction as a function of temperature;
3. Determine the temperature coefficient of the heat of reaction ΔСр at temperature T2 using graphical and analytical methods. Analyze the calculation results using the Kirchhoff equation;
4. Determine the change in entropy and normal affinity of the reaction at standard temperature. Analyze the obtained results;
5. Calculate the thermodynamic equilibrium constant of the reaction KT0 using the Temkin – Schwartzman method at temperatures T1, T2, T3. Analyze the obtained results based on the isobar of the chemical reaction;
6. Calculate the values ​​of rational equilibrium constants Kp, Kc, KN for a given reaction at temperature T2;
7. Based on the calculation data in p.5, plot a graph of the thermodynamic equilibrium constant versus temperature in coordinates lnKT0=f(1/T). Determine the heat of reaction at temperature T2 using the graphical method and compare the obtained value with the calculation results in p.2;
8. Calculate the equilibrium degree of conversion α and the mole fractions of the components of the equilibrium mixture Ni at temperature T2 and total pressure in the system Ptotal, if the starting materials were mixed in stoichiometric proportions and there are no reaction products in the starting mixture;
9. Explain the effect of the total pressure in the system and partial pressures on the standard equilibrium constant KT0, the equilibrium constant KN and the equilibrium degree of conversion.

№ Reaction equations T1, K T2, K T3, K Rob.105, Pa
1 CO2 3H2↔CH3OH H2O 450 500 600 2