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2 years ago

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Which direction will the following reaction (in a 5.0 L flask) proceed if the pressure of CO_2(g) is 1.0 atm? CaCO_3(s) rightarr

ow CaO(s) + C02(g) Kp = 1.9 times 10^-23
a. To the right because Q > K_p
b. To the right because Q < K_p
c. To the left because Q < K_p
d. To the left because Q > K_p

1 answer:

storchak [24]2 years ago

6 0

Answer:

d. To the left because Q > K_p

Explanation:

Hello,

In this case, for the given reaction:

$CaCO_3(s) \rightarrow CaO(s) + CO_2(g)$

The pressure-based equilibrium expression is:

$Kp=p_{CO_2}$

In such a way, since Kp is given we rather compute the reaction quotient at the specificed pressure of carbon dioxide as shown below:

$Q=p_{CO2}=1.0$

Therefore, since Q>Kp we can see that there are more products than reactants, which means that the reaction must shift leftwards towards the reactants in order to reestablish equilibrium, thus, answer is d. To the left because Q > Kp.

Regards.

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