Methane gas can be produced by the reaction of solid carbon with hydrogen gas as follows                     C(s)   +   2 H2(g)  ⇌   CH4(g)         Kp =  0.50 A vessel containing carbon is sealed and injected initially with hydrogen to a partial pressure of 2.0 atm and with methane to a partial pressure of 2.0 atm. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium?

Which of the following will affect the rate of a reaction? temperature of reaction magnitude of enthalpy of reaction (ΔH) concentration of reactants sign of enthalpy of reaction (ΔH) physical state of reactants

Consider the reaction of elemental bromine with elemental chlorine to make a bromochloride compound at 600 K:                                          Br2(g)  +  Cl2(g)   ⇌   2 BrCl(g)       KP = 81.0 A closed vessel at 600 K is charged with 3.00 atm of Br2(g) and 3.00 atm of Cl2(g) initially and allowed to reach equilibrium. What is the partial pressure of the BrCl (in atm) at that equilibrium?

For the following equilibrium CH4(g)  +   2 H2S(g)   ⇌   CS2(g)   +    4 H2(g) the equilibrium constant, K = 4.28  at 280.0 °C. Which of the following best describes the reaction at equilibrium?

The combustion of ammonia proceeds by the reaction           4 NH3    +    7 O2  →  4 NO2    +    6 H2O When the rate of appearance of H2O is 2.70 Ms-1, the rate of disappearance of O2 is          Ms-1

A sample of sodium bicarbonate, NaHCO3,  is placed in a closed 1.0 L vessel at 398 K and allowed to decompose unil it reaches equilibrium according to the following equation:                                         2 NaHCO3 (s)   ⇌  Na2CO3(s) +  H2O (g)   +  CO (g)      Kp = 0.250 What is the partial pressure of CO (in atm)  at equilibrium?

The following hypothetical reaction is zero order in A, second order in B, and first order in C: A +  B +  C  → products What is the correct rate law and the overall order of this reaction?    

Consider the following chemical reaction:                                    CO (g)  +  2 H2 (g)   ⇋   CH3OH (g)      Kc = 24.5 At equilibrium in a particular experiment, the concentrations of CO and H2 were 0.25 M and 0.78 M, respectively. What is the equilibrium concentration (in M) of CH3OH?  

The following hypothetical reaction is first order in A, second order in B, and zero order in C: A +  B +  C  → products What is the correct rate law and the overall order of this reaction?  

Given the equilibrium constant, Kc = 3.0 x 103 for the following reaction:           2 KCl (s)  +  3 O2(g)  ⇌  2 KClO3(s)  What is the concentration of O2 (in M) at equilibrium?