4. Given the reaction: PCls(g) = PC13(g) + Cl2(g) (AH° = +87.8 kJ/mol). Which of the following changes will cause the concentration of Cl2 to decrease? a. Increase the temperature. b. Add more PCI5 c. Compress the gas into a smaller volume. d. Remove PCI3. Add a catalyst. е. 5. Which of the ff. is NOT true about the activity coefficient? a. It increases as the concentration of electrolyte solution decreases. b. Higher activity coefficients correlate to lower ionic strength. c. It is the same for ions with the same charge. d. It departs away from unity as the charge of the ion increases. e. All are correct

4. Given the reaction: PCls(g) = PC13(g) + Cl2(g) (AH° = +87.8 kJ/mol). Which of the following changes will cause the concentration of Cl2 to decrease? a. Increase the temperature. b. Add more PCI5 c. Compress the gas into a smaller volume. d. Remove PCI3. Add a catalyst. е. 5. Which of the ff. is NOT true about the activity coefficient? a. It increases as the concentration of electrolyte solution decreases. b. Higher activity coefficients correlate to lower ionic strength. c. It is the same for ions with the same charge. d. It departs away from unity as the charge of the ion increases. e. All are correct

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following reaction: H₂(g) + CO (g) →→→ C(s) + H₂O (g) AH = 420 kJ/mol; K = 25; slow reaction Looking at the above information underline all the given parameters that are relevant to the equation and the given information. Example: Reversible because the reaction has double headed arrow A. Exothermic B. Reversible reaction C. Entropy (-AS) D. Large Ea E. Precipitate F. Supersaturated G. Reactant favored H. Endothermic
The following reversible chemical reaction shows the formation of nitrogen dioxide gas. How can you maximize how much nitrogen dioxide gas you make from this reaction. Select all that apply. 2NO(g) + O2(g) + heat ⇋ 2NO2(g) A.Remove products as they are produced B. Remove reactants C. Decrease temperature D. Increase pressure E. Decrease pressure F. Increase temperature
please highlight the correct answer and explain it
1. Given the following decomposition reaction: PCI5 (g) 2 PCI3 (g) + Cl2 (g) Predict the resulting direction of the shift in equilibrium when... AH° = 92.5 kJ/mol a. the temperature is raised b. more chlorine gas is added to the reaction mixture C. some PCI3 is removed from the mixture d. the pressure on the gases is increased e. a catalyst is added to the reaction mixture
10 For a chemical reaction: Cl2 (1) 0.55 mol Cl₂ Solve for the final partial pressure of Cl in atm: A. 1.8 × 108 B. 8.9 x 105 D. 3.6 × 104 2 Cl (g) has a Kp =3.2 x 10", and the initial amounts are: 0 atm Cl E. 0.55 C. 1.8 104 10.8
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
For the reaction below: A(g) > 2 B(g) Keg = 1.0 If you have 0.50 atm of A and 0.50 atm of B a. The reaction is at equilibrium b. The reaction is not at equilibrium and will move to the right c. The reaction is not at equilibrium and will move to the left.
DUE NOW. Please answer it all correctly.
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
For the following reaction, which of changes listed below would cause more reactants to form when equilibrium is re- established? 2NO(g) + Cl₂(g) 2NOCI(g) + 75 kJ a. Add a catalyst. b. Increase the volume. C. Increase the temperature. d. Decrease the [NO] e. Increase the pressure.
Which reaction, when at equilibrium, would be unaffected by a change in pressure? A. N2(g) + O2 (g) = 2NO(g) B. 2CO(g) + O2 = 2CO2(g) C. COBr2(g) = CO(g) + Br2(g) D. N2O4(g) = 2NO2 (g)
Consider the reaction: 2 CO2 (g) = 2 CO (g) + 02 (g). What will happen if the pressure is increased? We cannot predict O No effect O Shift to the left O Shift to the right