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Consider the following reaction:

$$2SO_2(g) + O_2(g) ⇄ 2SO_3(g)$$

...with concentrations of:

  • $SO_2(g) = 0.2 \text{ M}$
  • $O_2(g) = 0.5 \text{ M}$
  • $SO_3(g) = 0.7 \text{ M}$

...at equilibrium for a given temperature.

If the same reaction was completed using different concentrations:

  • $SO_2(g) = 0.1 \text{ M}$
  • $O_2(g) = 0.3 \text{ M}$
  • $SO_3(g) = 0.5 \text{ M}$

...which of the following would occur?

A

$K>Q$

The reaction will shift left.

B

$K < Q$

The reaction will shift left.

C

$K>Q$

The reaction will shift right.

D

$K < Q$

The reaction will shift right.

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