Task 1
1. Formulate the first law of thermodynamics and write its mathematical expression.
2. Write an equation for calculating the work of gas expansion in an ideal state at constant pressure, constant temperature, and constant volume.
3. Formulate Hess's law and write an equation that allows you to calculate the standard heat of a chemical reaction (ΔΗ0298).
4. For chemical reaction A (Table 5.1), based on the reference data given in the appendix (Table P1), determine the standard heat of reaction at 298 K and a standard pressure of 1.0132*105 Pa.
5. Determine the change in the number of moles of gaseous substances in this reaction (Δn).
6. Determine the heat of reaction at constant volume and 298 K (ΔU0298).
7. Formulate Kirchhoff's law and write its mathematical expression.
8. Calculate the heat effect of this chemical reaction at constant pressure and temperature T K, assuming that Cp ≠ f (T).
Option Chemical reaction A T, K
4 SO2 Cl2=SO2Cl2 600

THIS ALSO INCLUDES ASSIGNMENT 2,3,4,5, NAMELY:

Assignment 2
1. Formulate and write a mathematical expression for the second law of thermodynamics for reversible and irreversible processes.
2. Provide a definition of entropy.
3. Determine the change in entropy for chemical reaction A (Table 5.1) under standard conditions (ΔЅ0298) and at T, K (ΔЅ0Т). Reference data are provided in the appendix (Table P1).
Task 3
Calculate the change in entropy during heating (cooling) at constant pressure in the temperature range from T1 to T2 g kg of substance A (Table 5.2). Reference data are given in the appendix (Table P2).
Option No. Substance A g, kg T1, K T2, K
4 CH4O, methanol 80 303 473

Task 4
Calculate ΔG0 and ΔA0 at temperatures of 298 and T, K at P = const for the reaction given in Table 5.1 (task 1). Determine the direction of the reaction.
Task 5
1. List the signs of chemical equilibrium.
2. For the given chemical reaction A (Table 5.1), write in general form the expression for the constant of chemical equilibrium through the partial pressures, concentrations, and molar fractions of the reactants.
3. Based on the data from problem 4, determine the chemical equilibrium constant for reaction A (Table 5.1) at 298 and T, K. How will the numerical value of the equilibrium constant of the reaction change with increasing temperature?

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