Question

Be sure to answer all parts. As an EPA scientist studying catalytic converters and urban smog, you want to find Kc for the following reaction: 2 NO2(g) ⇌ N2(g) + 2 O2(g) Kc = ? Use the following data to find the unknown Kc: 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) Kc = 4.8 × 10 −10 2 NO2(g) ⇌ 2NO(g) + O2(g) Kc = 1.1 × 10−5 Kc = × 10

Answer 1

Answer:

Kc = 4.8x10^13

Explanation:

2 NO2(g) ⇌ N2(g) + 2 O2(g)

(1) 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) Kc = 4.8 × 10 −10

(2) 2 NO2(g) ⇌ 2NO(g) + O2(g) Kc = 1.1 × 10−5

Using the 2 given reactions you need to form the asked in the first place, in order to do that you multiply one of them by 2 and switch reactants with products and then add them together

(1): 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) / x2

N2(g) + O2(g) ⇌ 2 NO(g) / switch reactants with products (equivalent to multiply by -1)

2 NO(g) ⇌ N2(g) + O2(g)

(2): 2 NO2(g) ⇌ 2NO(g) + O2(g)

Adding them you get:

2 NO(g) + 2 NO2(g) ⇌ 2NO(g) + O2(g) + O2(g)

After eliminating NO in both sides:

2 NO2(g) ⇌ 2NO(g) + O2(g)

Now that the reaction is formed, everything you multiplied to the reactions you have to do the same in the constant but in the exponent and if you add reactions you multiply each other constants, then:

Kc = (4.8 × 10 −10)^(2*(-1)) *  1.1 × 10−5 = 4.8x10^13