In which one of the following processes is δh = δe? a. 2hi(g) => h2(g) + i2(g) at atmospheric pressure. b. two moles of ammonia gas are cooled from 325 ? °c to 300 °c at 1.2 atm. c. h2o(l) => h2o(g) at 100 °c at atmospheric pressure. d. caco3(s) => cao(s) + co2(g) at 800 °c at atmospheric pressure. e. co2(s) => co2(g) at atmospheric pressure.

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Explanation:

Formula used:

change in enthalpy

change in internal energy

change of moles

R = gas constant = 8.314 J / mol.K.

T = temperature

By the question, when value there will be zero.

Now we have the value of for the following cases.

(A) pushing the atmosphere.

In this case:

change of moles

Mole change = Number of moles on the product side – Number of moles on the reactant side

By reaction:

Mole change = (1 + 1) – 2 = 2 – 2 = 0 mole

That means, value = 0

So in this process

(B) Two moles of ammonia gas are cooled from 325 ° C to 300 ° C at 1.2 atm.

In this case:

change of moles

That means, value ≠ 0

So in this process

(C) at 100 ° C at atmospheric pressure.

In this case:

Mole change = Number of moles on the product side – Number of moles on the reactant side

By reaction:

Mole change = 1 – 0 = 1 mole

change of moles

That means, value ≠ 0

So in this process

(D) at 800 ° C at atmospheric pressure.

In this case:

Mole change = Number of moles on the product side – Number of moles on the reactant side

By reaction:

Mole change = 1 – 0 = 1 mole

change of moles

That means, value ≠ 0

So in this process

(E) pushing the atmosphere.

In this case:

Mole change = Number of moles on the product side – Number of moles on the reactant side

By reaction:

Mole change = 1 – 0 = 1 mole

change of moles

That means, value ≠ 0

So in this process

Accordingly, we are of the view that only option A is shown for this