Chemistry

Problem

For the equilibrium

2\text{NO}_2(g)\;\rightleftharpoons\;\text{N}_2\text{O}_4(g)

K_c

1.7

at 400 K and

0.30

at 500 K. A sealed flask is heated to 500 K and contains

[\text{NO}_2]=0.40\,\text{M}

and

[\text{N}_2\text{O}_4]=0.12\,\text{M}

. Which option gives the value of

Q_c

at 500 K and predicts how the system will shift to reach equilibrium at that temperature? a)

Q_c = 0.30;\,

the system is already at equilibrium. b)

Q_c = 1.3;\,

the reaction will form more NO

_2

. c)

Q_c = 0.75;\,

the reaction will form more NO

_2

. d)

Q_c = 0.75;\,

the reaction will form more N

_2

_4