Questions: Consider the following reaction: 3 H2(g) + N2(g) ⇌ 2 NH3(g) K=4.3 × 10^-4 Part 1 of 5 Write the expression for the equilibrium constant for this reaction. K=

Consider the following reaction:
3 H2(g) + N2(g) ⇌ 2 NH3(g) K=4.3 × 10^-4

Part 1 of 5

Write the expression for the equilibrium constant for this reaction.
K=

Transcript text: Consider the following reaction: \[ 3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \quad K=4.3 \times 10^{-4} \] Part: $0 / 5$ Part 1 of 5 Write the expression for the equilibrium constant for this reaction. \[ K= \] $\square$

Solution

Solution Steps

Step 1: Identify the reaction and equilibrium constant expression

The given reaction is: \[ 3 \mathrm{H}_{2}(g) + \mathrm{N}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \] We need to write the expression for the equilibrium constant $ K $.

Step 2: Write the general form of the equilibrium constant expression

For a general reaction of the form: \[ aA + bB \rightleftharpoons cC + dD \] The equilibrium constant $ K $ is given by: \[ K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]

Step 3: Apply the general form to the given reaction

For the given reaction: \[ 3 \mathrm{H}_{2}(g) + \mathrm{N}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \] The equilibrium constant expression is: \[ K = \frac{[\mathrm{NH}_3]^2}{[\mathrm{H}_2]^3 [\mathrm{N}_2]} \]