a mixture of 4.1 atm $\text{co}_2$, 2.1 atm $\text{h}_2$, and 3.3 atm $\text{h}_2\text{o}$ are added to a 2.0 l vessel at 500 k and allowed to come to equilibrium. at equilibrium, there are 3.5 atm of $\text{h}_2\text{o}$.

$\begin{array}{lccccc}
\text{r} & \text{co}_2(g) & + & \text{h}_2(g) & \
ightleftharpoons & \text{co}(g) & + & \text{h}_2\text{o}(g) \\
\text{i} & 4.1 & & 2.1 & & 0 & & 3.3 \\
\text{c} & & & & & & & \\
\text{e} & & & & & & & 3.5
\end{array}$

what is the pressure of $\text{co}$ at equilibrium?
$p_{\text{co}} = ?\text{ atm}$

Question

a mixture of 4.1 atm $\text{co}_2$, 2.1 atm $\text{h}_2$, and 3.3 atm $\text{h}_2\text{o}$ are added to a 2.0 l vessel at 500 k and allowed to come to equilibrium. at equilibrium, there are 3.5 atm of $\text{h}_2\text{o}$.

$\begin{array}{lccccc}
\text{r} & \text{co}_2(g) & + & \text{h}_2(g) & \
ightleftharpoons & \text{co}(g) & + & \text{h}_2\text{o}(g) \\
\text{i} & 4.1 & & 2.1 & & 0 & & 3.3 \\
\text{c} & & & & & & & \\
\text{e} & & & & & & & 3.5
\end{array}$

what is the pressure of $\text{co}$ at equilibrium?
$p_{\text{co}} = ?\text{ atm}$

Accepted Answer

{ "quality": "clear", "question_count": 1, "skills_matched": [ "step_cot", "blank_filling_formatter", "explain_then_answer", "tutor", "mastery_adaptive_brevity" ], "needs_drawing": false, "concepts_used": [ "RICE Table Calculations", "Partial Pressure Equilibrium" ], "new_concepts": [], "current_concepts": [ "RICE Table Calculations", "Partial Pressure Equilibrium", "Chemical Equilibrium" ] } ## Identify the change in pressure for water vapor Using the *RICE Table Calculations* and *Partial Pressure Equilibrium* knowledge points $$ \begin{aligned} P_{\mathrm{H_2O, \, initial}} &= 3.3\text{ atm} \ P_{\mathrm{H_2O, \, equilibrium}} &= 3.5\text{ atm} \ x &= P_{\mathrm{H_2O, \, equilibrium}} - P_{\mathrm{H_2O, \, initial}} = 3.5 - 3.3 = 0.2\text{ atm} \end{aligned} $$ ## Determine the equilibrium pressure of carbon monoxide Using the *RICE Table Calculations* and *Partial Pressure Equilibrium* knowledge points $$ \begin{aligned} P_{\mathrm{CO, \, initial}} &= 0\text{ atm} \ P_{\mathrm{CO, \, equilibrium}} &= P_{\mathrm{CO, \, initial}} + x = 0 + 0.2 = 0.2\text{ atm} \end{aligned} $$ A mixture of $4.1\text{ atm }\mathrm{CO_2}$, $2.1\text{ atm }\mathrm{H_2}$, and $3.3\text{ atm }\mathrm{H_2O}$ are added to a $2.0\text{ L}$ vessel at $500\text{ K}$ and allowed to come to equilibrium. At equilibrium, there are $3.5\text{ atm}$ of $\mathrm{H_2O}$. What is the pressure of $\mathrm{CO}$ at equilibrium? $P_{\mathrm{CO}} =$ 0.2 atm { "subject": "Natural Science", "question_type": "Fill-in-the-blank", "knowledge_point": [ "Natural Science", "Chemistry", "Chemical Equilibrium" ] }

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Question

Explanation:

Identify the change in pressure for water vapor

Determine the equilibrium pressure of carbon monoxide

Answer: