Questions: Chapter 6 Homework Question 22 of 24 (1 point) I Question Attempt: 3 of Unlimited Raisha =22 Methanol (CH4O) is used as a fuel in race cars. Gaseous methanol burns in oxygen (O2) to form carbon dioxide, CO2, and water vapor, H2O. Part 1 of 6 Write a balanced equation for this equilibrium. Include all physical states of matter. 2 CH4O(g)+3 O2(g) ⇌ 2 CO2(g)+4 H2O(g) Part 2 of 6 Write the expression for the equilibrium constant for this reaction.

Chapter 6 Homework
Question 22 of 24 (1 point) I Question Attempt: 3 of Unlimited
Raisha

=22

Methanol (CH4O) is used as a fuel in race cars. Gaseous methanol burns in oxygen (O2) to form carbon dioxide, CO2, and water vapor, H2O.

Part 1 of 6

Write a balanced equation for this equilibrium. Include all physical states of matter.

2 CH4O(g)+3 O2(g) ⇌ 2 CO2(g)+4 H2O(g)

Part 2 of 6

Write the expression for the equilibrium constant for this reaction.

Transcript text: www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IBIk_Z5zNtWHhRgilODc5MqvhZbKYx2-U-03j_IWxnm8qVVt0PILOZthKVAgAaOzcUnFeRs1SpvpGb Chapter 6 Homework Question 22 of 24 (1 point) I Question Attempt: 3 of Unlimited Raisha 12 13 14 15 16 18 20 21 $=22$ 23 Methanol $\left(\mathrm{CH}_{4} \mathrm{O}\right)$ is used as a fuel in race cars. Gaseous methanol burns in oxygen $\left(\mathrm{O}_{2}\right)$ to form carbon dioxide, $\mathrm{CO}_{2}$, and water vapor, $\mathrm{H}_{2} \mathrm{O}$. Part 1 of 6 Write a balanced equation for this equilibrium. Include all physical states of matter. \[ 2 \mathrm{CH}_{4} \mathrm{O}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}_{2}(\mathrm{~g})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \] Part 2 of 6 Write the expression for the equilibrium constant for this reaction. $\square$

Solution

Solution Steps

Step 1: Understanding the Reaction

The given reaction is the combustion of methanol in oxygen to form carbon dioxide and water vapor. The balanced chemical equation is: \[ 2 \mathrm{CH}_{4} \mathrm{O}(\mathrm{~g}) + 3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}_{2}(\mathrm{~g}) + 4 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \]

Step 2: Writing the Equilibrium Constant Expression

The equilibrium constant expression, $ K_c $, for a reaction is given by the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective coefficients in the balanced equation.

For the reaction: \[ 2 \mathrm{CH}_{4} \mathrm{O}(\mathrm{~g}) + 3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}_{2}(\mathrm{~g}) + 4 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \]

The equilibrium constant expression is: \[ K_c = \frac{[\mathrm{CO}_{2}]^2 [\mathrm{H}_{2} \mathrm{O}]^4}{[\mathrm{CH}_{4} \mathrm{O}]^2 [\mathrm{O}_{2}]^3} \]