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Standard XI
Chemistry
Ideal Gas Equation
Question
At $$973$$ K, $$K_p$$ is $$1.50$$ for the reaction:
$$C(s) + CO_2(g) \rightleftharpoons \ 2CO(g)$$
Suppose the total gas pressure at equilibrium is $$1.0$$ atm. What are the partial pressures of $$CO$$ and $$CO_2$$?
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Solution
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At equilibrium,
$$C(s) + \underset{P_1}{CO_2(g)} \rightleftharpoons \underset{P_2(say)}{2CO(g)} \ \ \ \ Kp = 1.5$$
$$Kp = \cfrac{P_2^2}{P^1} = 1.5 \Rightarrow P_2^2 = 1.5 P_1$$
Also $$P_1 + P_2 = 1$$
$$P_2 = 1 - P_1$$
$$P_2^2 = 1 + P_1^2 - 2P_1 = 1.5 P_1$$
$$ 1 + P_1^2 -3.5 P_1 = 0$$
$$P_1 = 0.314 atm \Rightarrow P_{CO_2} = 0.314 atm$$
$$P_2 = 0.686 atm \Rightarrow P_{CO} = 0.686 atm$$
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Similar Questions
Q1
At $$973$$ K, $$K_p$$ is $$1.50$$ for the reaction:
$$C(s) + CO_2(g) \rightleftharpoons \ 2CO(g)$$
Suppose the total gas pressure at equilibrium is $$1.0$$ atm. What are the partial pressures of $$CO$$ and $$CO_2$$?
View Solution
Q2
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C
(
s
)
+
C
O
2
(
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⇌
2
C
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g
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, the partial pressure of
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O
are
2.0
and
4.0
atm, respectively.
At equilibrium the
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p
of the reaction is:
View Solution
Q3
For the reaction,
C
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s
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+
C
O
2
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g
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⇌
2
C
O
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g
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, the partial pressure of
C
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and
C
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Q4
For the reaction
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2
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g
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→
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C
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O
2
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C
O
are
2.0
and
4.0
atm respectively. At equilibrium the
K
p
for the reaction is.
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Q5
For the reaction
C
(
s
)
+
C
O
2
(
g
)
⇌
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C
O
(
g
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,
the partial pressure of
C
O
2
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