Chem Worksheet

Question 1 Consider the following equilibrium.4NH3(g) + 3O2(g) | View Full Image | | 2N2(g) + 6H2O(g)Suppose 0.30 mol of NH3 and 0.40 mol of oxygen are added to a 5.0-L container. If x mol of water is present at equilibrium, what is the equilibrium concentration of oxygen?Answer 0.40 - 0.50x | 0.30 - 0.50x | 0.08 - 0.10x | 0.06 - 0.13x | 0.40 - | View Full Image | | x |
4 points
Question 2 At 298 K, the value of Kc for the reaction H2(g) + Br2(g) | View Full Image | | 2HBr(g) is 2.0 × 1019. What is Kc for HBr(g) | View Full Image | | ½H2(g) + ½Br2(g)?Answer -2.0 × 1019 | 5.0 × 10-20 | 2.2 × 10-10 | 4.0 × 10-38 | 1.0 × 1019 |
4 points
Question 3 Consider the following equilibrium:2NH3(g) | View Full Image | | N2(g) + 3H2(g); ΔH = 92 kJWhat change should be made in order to increase the value of Kp for this reaction? Answer Increase the temperature. | Decrease the temperature. | Increase the pressure. | Decrease the pressure. | Nothing; Kp cannot be changed. |
4 points
Question 4 One method for the decomposition of carbon dioxide proceeds as follows:2CO2(g) | View Full Image | | 2CO(g) + O2(g); ΔH= 559 kJWhich of the following changes will cause an increase in the equilibrium concentration of CO?Answer increasing the pressure of the system at constant temperature | adding more O2 to the system | removing CO2 from the system | increasing the temperature of the system | adding a catalyst |
4 points
Question 5 Which of the following correctly describes the equilibrium constant for the gas-phase reaction between H2 and O2 to form gaseous H2O?Answer Kc = | View Full Image | | | Kc = | View Full Image | | | Kc = | View Full Image | | | Kc = | View Full Image |