Question

At a certain temperature, the equilibrium constant K for the following reaction is 4.3 x 10': NO2(g) + NO(g) = 2 NO2(g) Use this information to complete the following table. There will be very little NO3 and NO. Suppose a 41. L reaction vessel is filled with 0.79 mol of NO2. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO2. x 6 ? O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 NO2(9) = NO3(9)+NO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 1 3 NO3(9)+3NO(g) = 6NO2(9)

Answer 1

a. Since equilibrium constant of rxn a is very high so reaction almost go to completion , so vert little amount of reactant will be present at equilibrium.

NO2 g NO3 g) + Now) K= 4.3x10? ( 2002 - NO3(g) + NOG) (NO₃] [ro] [N]2 4.3x10 7 = 0.233x107 = 2.33x10" K In a = 2.33 x 10 significant sigese figure K'= 2.3x107 (c). 3N03 (g) + 300g) - 6 NO 2 (g) K" = (K) (since son has been multiplied (413 vict) by 3) 79.504 x4021 = In 2 22 = 7.9507 x 10² significant digit k" = 8.0 x 1022 (O.o) J" = 80 x 1022