Consider the system at equilibrium.
2CO(g)+O2(g)<--->2CO2(g)
A. How will increasing the concentration of CO shift the equilibrium?
B. How will increasing the concentration of Co, shift the equilibrium?
C. How will adding a catalyst shift the equilibrium?
Consider the system at equilibrium. 2 CO(g) +0,(g) = 200,(g) A. How will increasing the concentration...
Consider the following system at equilibrium. 2co a) How will increasing the concentration of CO shift the equilibrium? O to the right O to the left O no effect b) How will increasing the concentration of CO2 shift the equilibrium? O to the right O to the left O no effect c) How will decreasing the the volume of the container shift the equilibrium? O to the right O to the left O no effect
1. The oxidation of carbon monoxide proceeds as follows: 2CO(g) + O2(g) 2CO2(g) + 559 kJ Which of the following will cause an INCREASEin the equilibrium concentration of CO? a. decreasing the pressure of the system at constant temperature b. adding more O2to the system c. removing CO2from the system as it is formed d. increasing the pressure of the system at constant temperature e. adding a catalyst
Consider the following system at equilibrium. PCI A. How will increasing the concentration of PCls shift the equilibrium? O to the left O no effect O to the right B. How will increasing the concentration of PCl3 shift the equilibrium? O to the right O to the left O no effect C. How will increasing the pressure by adding argon gas to the reaction mixture, while maintaining a constant volume, shift the equilibrium O to the left O to the...
16. For the system CO + CO2(g) → CaCO(s) the equilibrium constant expression is a. [CO] b. 1/[CO] c. COCO/CaCO, d. Cacos/CaoCO 17. The value of K, for the reaction 2NOH). N204) is 1.52 at 319 K. What is the value of ko at this temperature for the reaction N04() → 2NOR ? b. 1.23 c. 5.74 x 10 d. 0.658 18. The value of Ke for the reaction C() + COX() -----2CO(g) is 1.6. What is the equilibrium concentration...
For each event, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. 2CO(g) + O2(g) ↽−−⇀ 2CO2(g) increasing the concentration of CO increasing the concentration of CO2 decreasing the volume of the system
200(g) + 0,(8) 200,(8) increasing the concentration of CO increasing the concentration of CO, OOO decreasing the volume of the system Answer Bank
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
. Consider the chemical system: 2NO(g) + O2(g) <---> 2NO2(g) Fill in the blanks. An increase in pressure will cause the equilibrium to shift to the ___(1)___, increasing the concentration of _____(2)____ and decreasing the concentration of _____(3)___. The reaction is endothermic. A decrease in temperature will cause the equilibrium to shift to the ____(1)_____, increasing the concentration of ___(2)____, and decreasing the concentration of ____(3)____. Removal of O2 will cause the equilibrium to shift to the____(1)_____, increasing the concentration...
At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g) <----> 2CO(g) +O2(g) are 1.6*10^-11 and 1.3*10^-10, respectively. a. what is the value of the equilibrium constant for the reaction: (3) CO2(g) + H2(g) <----> H2O(g) + CO(g) at this temperature? b. demonstrate how the calculations of equilibrium constants matches the calculations of dG0r when adding two reactions or more ; determine dG0r for reactions (1) and (2) and use these values in order...
Consider the following reaction at equilibrium: 2CO2(g) = 200 (g) + O2(g) AH° = -514 kJ Le Châtelier's principle predicts that a decrease in temperature will decrease the value of the equilibrium constant O increase the value of the equilibrium constant decrease the partial pressure of CO increase the partial pressure of CO2 (g) decrease the partial pressure of O2 (g) Consider the following reaction at equilibrium: 2NH3 (g) = N2 (g) + 3H2(g) AH° = +92.4 kJ Le Châtelier's...