The industrial production of lime (CaO ) from calcium carbonate is accomplished

ID: 903583 • Letter: T

Question

The industrial production of lime (CaO ) from calcium carbonate is accomplished via the following reaction:

CaCO3(s)CaO(s)+CO2(g)

Given the following data:

what can be said about this reaction?

The equilibrium lies far to the right at room temperature.

Given the following data:

what can be said about this reaction?

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Part C

For the reaction

2CO2(g)2CO(g)+O2(g) , K= 1.00×1013 at 1200 K

what can be said about this reaction at this temperature?

For the reaction

m 2CO_2(g) ightleftharpoons 2CO(g) + O_2(g), {it K} = m 1.00 imes10^{-13} at 1200 m K

what can be said about this reaction at this temperature?

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Part D

For the reaction

HCONH2(g)NH3(g)+CO(g) , K= 4.84 at 400 K

what can be said about this reaction at this temperature?

Temperature
(K ) K 298 1.93×1023 1200 1.01

From the given data of lime formation we say that at T = 1200

Equilibrium constant of the reaction = 1

This shows that formation of product increases with increasing T

So the answer is

b. The reaction makes more lime at higher temperature.

Part C

The same is true for this reaction

For this reaction, If we increase the temperature more product is formed.

So answer is

b. The reaction makes more product.

Part D

The equilibrium constant at 400 K is 4.84 .

This suggest that there is more product than the reactant so the answer is

c. The reaction contains significant amount of product at equilibrium.

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