10 g of hydrogen gas and 355 g of chlorine gas are heated together in a sealed 500 cm³ container. A chemical equilibrium is reached at 450 °C. The balanced equation for the reaction is: H₂(g) + Cl₂(g) ⇌ 2HCl(g). The equilibrium constant Kc for this reaction at 450 °C is 64.

June 4, 2026Chemistry

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June 4, 2026

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10 \text{ g}$

6.1 The balanced equation for the reaction is: $\text{H}_2(g) + Cl_2(g) \rightleftharpoons 2HCl(g)$ Given: Mass of $\text{H}_2 = 10 \text{ g}$ Mass of $\text{Cl}_2 = 355 \text{ g}$ Volume of container = $500 cm^3 = 0.5 dm^3$ Equilibrium constant $K_c = 64$ at $450 \text{ °C}$

Step 1: Calculate the initial moles of

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6.1 The balanced equation for the reaction is: H_2(g) + Cl_2(g) 2HCl(g) Given: Mass of H_2 = 10 g Mass of Cl_2 = 355 g Volume of container = 500 cm^3 = 0.5 dm^3 Equilibrium constant K_c = 64 at 450 °C Step 1: Calculate the initial moles of ✂️ _That an…

Asked on June 4, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

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6.1 The balanced equation for the reaction is: H_2(g) + Cl_2(g) 2HCl(g) Given: Mass of H_2 = 10 g Mass of Cl_2 = 355 g Volume of container = 500 cm^3 = 0.5 dm^3 Equilibrium constant K_c = 64 at 450 °C Step 1: Calculate the initial moles of ✂️ _That answer was long and got cut off. Reply continue and I'll finish it._

10 g of hydrogen gas and 355 g of chlorine gas are heated together in a sealed 500 cm³ container. A chemical equilibrium is reached at 450 °C. The balanced equation for the reaction is: H₂(g) + Cl₂(g) ⇌ 2HCl(g). The equilibrium constant Kc for this reaction at 450 °C is 64.

June 4, 2026Chemistry