For the chemical equation SO 2 ( g ) + NO 2 ( g ) − ⇀ ↽ − SO 3 ( g ) + NO ( g ) SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium co

Question

3 months ago

12

For the chemical equation SO 2 ( g ) + NO 2 ( g ) − ⇀ ↽ − SO 3 ( g ) + NO ( g ) SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium co

nstant at a certain temperature is 2.70 . 2.70. At this temperature, calculate the number of moles of NO 2 ( g ) NO2(g) that must be added to 2.99 mol SO 2 ( g ) 2.99 mol SO2(g) in order to form 1.30 mol SO 3 ( g ) 1.30 mol SO3(g) at equilibrium.

Chemistry

1 answer:

lions [2.9K] · Answer 1 · 2026-03-01T15:44:55+03:00

Answer: The calculated moles of $NO_2$ that need to be added is 0.37 mol.

Explanation:

The chemical equation in question is:

$SO_2(g)+NO_2(g)\rightleftharpoons SO_3(g)+NO(g)$

Initially, the molar quantities are as follows: 2.99, x, 0, 0

At equilibrium: (2.99-1.30), (x-1.30), 1.30, 1.30

= 1.69.

The equation for the equilibrium constant is given by:

$K_c=\frac{[SO_3][NO]}{[SO_2][NO_2]}$

Now substituting the provided values into this equation yields:

$2.70=\frac{(1.30)\times (1.30)}{(1.69)\times (x-1.30)}$

x = 1.67 mol.

The moles of $NO_2$ needed to be added is (x-1.30) = (1.67-1.30) = 0.37 mol.