Question

Part B The following reaction was performed in a sealed vessel at 735 °C: $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ Initially, only $H_2$ and $I_2$ were present at concentrations of $[H_2] = 3.45M$ and $[I_2] = 2.90M$. The equilibrium concentration of $I_2$ is 0.0800 M. What is the equilibrium constant, $K_c$, for the reaction at this temperature? Express your answer numerically. $K_c = $

          Part B
The following reaction was performed in a sealed vessel at 735 °C:
$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$
Initially, only $H_2$ and $I_2$ were present at concentrations of $[H_2] = 3.45M$ and $[I_2] = 2.90M$. The equilibrium concentration of $I_2$
is 0.0800 M. What is the equilibrium constant, $K_c$, for the reaction at this temperature?
Express your answer numerically.
$K_c = $

Part B
The following reaction was performed in a sealed vessel at 735 °C:
H2(g) + I2(g) ⇌ 2HI(g)
Initially, only H2 and I2 were present at concentrations of [H2] = 3.45M and [I2] = 2.90M. The equilibrium concentration of I2
is 0.0800 M. What is the equilibrium constant, Kc, for the reaction at this temperature?
Express your answer numerically.
Kc =

Added by Jesse T.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

09/25/2023

Step 1

$$K_c = \frac{[HI]^2}{[H_2][I_2]}$$ Show more…

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Part B The following reaction was performed in a sealed vessel at 735 °C: H2(g) + I2(g) 2HI(g) Initially, only H2 and I2 were present at concentrations of [H2] = 3.45M and [12] = 2.90M. The equilibrium concentration of I2 is 0.0800 M. What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically. ► View Available Hint(s) Kc = Submit