A gaseous mixture contains 0.30 moles CO, 0.10 moles H2, and 0.03 moles H2 O vapour and an unkno

step 1 Hello everyone so in this question there is a reaction given that is carbon dioxide reacts with

A gaseous mixture contains 0.30 moles CO, 0.10 moles H2, and...

A gaseous mixture contains $0.30$ moles $\mathrm{CO}, 0.10 \mathrm{moles} \mathrm{H}_{2}$, and $0.03$ moles $\mathrm{H}_{2} \mathrm{O}$ vapour and an unknown amount of $\mathrm{CH}_{4}$ per litre. This mixture is at equilibrium at $1200 \mathrm{~K}$. $\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ $K_{\mathrm{C}}=3.9$ What is the concentration of $\mathrm{CH}_{4}$ in this mixture? The equilibrium constant $K_{\mathrm{c}}$ equals $3.92$. (a) $0.39 \mathrm{M}$ (b) $0.039 \mathrm{M}$ (c) $0.78 \mathrm{M}$ (d) $0.078 \mathrm{M}$

A gaseous mixture contains $0.30$ moles $\mathrm{CO}, 0.10 \mathrm{moles} \mathrm{H}_{2}$, and $0.03$ moles $\mathrm{H}_{2} \mathrm{O}$
vapour and an unknown amount of $\mathrm{CH}_{4}$ per litre. This mixture is at equilibrium at $1200 \mathrm{~K}$.
$\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
$K_{\mathrm{C}}=3.9$
What is the concentration of $\mathrm{CH}_{4}$ in this mixture? The equilibrium constant $K_{\mathrm{c}}$ equals $3.92$.
(a) $0.39 \mathrm{M}$
(b) $0.039 \mathrm{M}$
(c) $0.78 \mathrm{M}$
(d) $0.078 \mathrm{M}$

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the forward and reverse reaction rates are equal, causing the concentrations of reactants and products to remain constant over time. This concept is central to understanding how systems adjust when conditions such as concentration, temperature, or pressure change.

Equilibrium Constant (Kc)

The equilibrium constant, denoted as Kc when expressed in terms of concentration, is a numerical value that relates the concentrations of products and reactants at equilibrium, each raised to the power of their stoichiometric coefficients. It provides insight into the extent of a reaction and helps predict the position of equilibrium.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation to determine the quantitative relationships between reactants and products. In equilibrium problems, stoichiometry helps in setting up the equilibrium expression correctly, ensuring that the concentration terms are raised to the appropriate powers corresponding to their coefficients.

Algebraic Manipulation of Equilibrium Expressions

Algebraic manipulation of equilibrium expressions involves substituting known concentrations and the given equilibrium constant into the equilibrium expression, followed by rearranging and solving for the unknown concentration. This systematic approach is a crucial skill in quantitative chemical equilibrium analysis.

Transcript

Please give Ace some feedback