reactions

For which of the following reactions does Kc equal Kp? a. C2H4(g)+H2(g) (equilibrium sign) C2H6(g) b. H2(g)+l2(s) (equilibrium sign) 2Hl(g) c. 2S(s)+3O2(g) (equilibrium sign) 2SO3(g) d. SO2(g)+NO2(g) (equilibrium sign) SO3(g)+NO(g) e. both answers b and d

equilibrium

For the reaction below, the partial pressures of gases at equilibrium are as follows: H2=7.1x10(exponent negative 5)atm, Cl2=2.5x10(exponent negative 6)atm, and HCl=3.0atm. What is the value of the equilibrium constant Kp? H2(g)+Cl2(g) (equilibrium sign) 2HCl(g)

equilibrium constant

Nitrosyl chloride decomposes according to this reaction: 2NOCl(g) (equilibrium sign) 2NO(g)+Cl2(g) 0.600 atm of nitrosyl chloride is sealed in a flask and alowed to reach equilibrium. If 27% of the NOCl decomposes, what is the equlibrium constant for the reaction? a. 0.00485 b. 0.781 c. 0.0300 d. 0.370 e. 0.0111

Multiple choice question about the equilibrium partial pressure of a gas.

For the system CO(g)+H2O(g) <--> CO2(g)+H2(g) Kp is 1.6 at 900K. If 0.500 atm CO(g) and 0.500 atm H2O(g) are combined in a sealed flask, what is the equilibrium partial pressure of CO2(g)? a. 0.279 atm b. 0.308 atm c. 0.471 atm d. 0.608 atm e. 0.942 atm

reactions

Which of the following statement is true? a. Increasing the temperature of the reaction will always result in higher product yields b. catalysts shift the equilibrium constant in favor of the products c. Kc and kp are the same for gas phase reactions d. Increasing the volume of a system(at constant temperature) will change the equilibrium constant in favor of the side of the reaction with more particles e. Equilibrium is established when the forward and backward rates of reaction are equal