Final answer:
To calculate the number of moles of NO₂(g) that must be added to 3.08 moles of SO₂(g) in order to form 1.40 moles of SO₃(g) at equilibrium, we can use the equilibrium constant (K) formula. Plugging in the given values, we can solve for the unknown, which is [NO₂]. The moles of NO₂(g) that must be added is approximately 0.1297 moles.
Step-by-step explanation:
The equilibrium constant (K) for the chemical equation SO₂ (g) + NO₂(g) ⇄ SO₃(g) + NO(g) is given as 3.50. To calculate the number of moles of NO₂(g) that must be added to 3.08 moles of SO₂(g) in order to form 1.40 moles of SO₃(g) at equilibrium, we can use the equation: K = ([SO₃] * [NO]) / ([SO₂] * [NO₂]). Plugging in the given values into the equation, we can solve for the unknown, which is [NO₂].
Using the given values:
[SO₂] = 3.08 moles
[NO₂] = unknown
[SO₃] = 1.40 moles
[NO] = unknown
Plugging in the values into the equation, we get:
3.50 = (1.40 * unknown) / (3.08 * unknown)
Simplifying the equation, we have:
3.50 * (3.08 * unknown) = 1.40 * unknown
10.784 * unknown = 1.40 * unknown
10.784 = 1.40
unknown = 1.40 / 10.784
unknown = 0.1297
Therefore, approximately 0.1297 moles of NO₂(g) must be added to 3.08 moles of SO₂(g) to form 1.40 moles of SO₃(g) at equilibrium.