At a particular temperature, K = 3.75 for the following reaction.
SO2(g) + NO2(g) SO3(g) + NO(g)
If all four gases had initial concentrations of 0.520 M, calculate the equilibrium concentrations of the gases
2 answers
332 over 64
How can you have an equation with no arrow. What are the products and what are the reactants? I will assume it it
SO2(g) + NO2(g) ==>SO3(g) + NO(g)
Step 1. Determine which way the the reaction must go to reach equilibrium. Determine the reaction quotient.
Q = (SO3)(NO)/(SO2)(NO2)
(0.520)(0.520)/(0.520)(0.520) = 1
K = 3.75 which is greater than Q; therefore, Q is too small. That means the numerator is too small and the denominator is too large so products are too small and reactants too large. The reaction must go to the right to reach equilibrium.
Prepare an ICE chart and solve for individual concns.
Post your work if you get stuck.
SO2(g) + NO2(g) ==>SO3(g) + NO(g)
Step 1. Determine which way the the reaction must go to reach equilibrium. Determine the reaction quotient.
Q = (SO3)(NO)/(SO2)(NO2)
(0.520)(0.520)/(0.520)(0.520) = 1
K = 3.75 which is greater than Q; therefore, Q is too small. That means the numerator is too small and the denominator is too large so products are too small and reactants too large. The reaction must go to the right to reach equilibrium.
Prepare an ICE chart and solve for individual concns.
Post your work if you get stuck.
4 answers