A cylinder contains 4 mol of an ideal gas at 30^oC.  If it expands from an initial volume of 1.0 m³ to 2.0 m³ while maintained at a constant pressure of 200 kPa.

1. What is the change in the temperature of the gas?
2. How much heat is absorbed or released from the system, over the process?  

The pressure is then reduced while the gas is held at a constant volume.

3. If over this process the gas is returned to its original temperature, what is the heat absorbed or released, over that process?

2. Use the following data (measured at 1200 K) to estimate the value of Kp at 1200 K for the reaction:

2H2(g) + O2(g) ↔ 2H2O(g)
Data:

C(graphite) + CO2(g) ↔ 2CO(g) Kc = 0.64
CO2(g) + H2(g) ↔ CO(g) + H2O(g) Kc = 1.4
C(graphite) + 1/2 O2(g) ↔ CO(g) Kc = 1.0 x 108

AgNO₃ is slowly added to an aqueous solution containing 0.02 M AsO₄^3-, 0.02 M I^- and 0.02 M CO₃^2-. In what order would the silver salts precipitate?

K_sp( Ag₃AsO₄)= 1.0 x 10^-22

K_sp (AgI) = 8.3 x 10^-17

K_sp (Ag₂CO₃)= 8.1 x 10^-12

Determine the calorimeter heat capacity using the known enthalpy of combustion of benzoic acid.

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0 L vessel at 300 K. At equilibrium [NO] = 0.062 M.

2 NO(g) + 2H2 ⇌ N2(g) + 2 H2O(g)

a. What is the Kc at 300 K?

b. What is the Kc of the halved reaction, given, at 300 K?

NO(g) + H2 ⇌ ½ N2(g) + H2O(g)

c. What is the Kp of part (a) at 300 K?

d. What is the Kc of the reaction if reversed?

For the reaction below, K = 5.0×1033 at 298 K. [AuCl4]−(aq) + 3 V3+(aq) + 3 H2O(l) Au(s) + 4 Cl−(aq) + 3 VO2+(aq) + 6 H+(aq) In an experiment, 0.50 mol of KAuCl4 and 0.50 mol of V(ClO4)3 are dissolved in water at 298 K to make 1.0 L of solution. Calculate the equilibrium concentrations of all ionic species. Justify any approximations you make.

Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K.

3 significant figures in answer.

A. 2NO2(g)⇌N2O4(g) ΔH∘f for N2O4(g) is 9.16 kJ/mol.

B. Br2(g)+Cl2(g)⇌2BrCl(g) ΔH∘f for BrCl(g) is 14.6 kJ/mol.

A 10-cm-long thin glass rod uniformly charged to 7.00 nCnC and a 10-cm-long thin plastic rod uniformly charged to - 7.00 nCnC are placed side by side, 4.10 cmcm apart. What are the electric field strengths E1E1 to E3E3 at distances 1.0 cm, 2.0 cm, and 3.0 cm from the glass rod along the line connecting the midpoints of the two rods?

Specify the electric field strength E1, E2, and E3?

Consider the following equilibrium system at 25°C and select the true statement below:

HA(aq) + H2O(l) ↔ H3O+(aq) + A−(aq)        Ka = 1.0 x 10−4 at 25°C

this is a product-favored system at 25°C

a solution of NaA(s) dissolved in pure water is predicted to have a pH < 7.00 at 25°C

(Kb of A−) = 1 / (Ka of HA)

A− is a stronger base than H2O

HA is a stronger acid than H3O+

A 10-cm-long thin glass rod uniformly charged to 7.00 nCnC and a 10-cm-long thin plastic rod uniformly charged to - 7.00 nCnC are placed side by side, 4.10 cmcm apart. What are the electric field strengths E1E1 to E3E3 at distances 1.0 cm, 2.0 cm, and 3.0 cm from the glass rod along the line connecting the midpoints of the two rods?

Specify the electric field strength E1, E2, and E3.