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HIGH SCHOOL CHEMISTRY 25 PTS
Consider the following intermediate chemical equations.

3 equations. 1: upper C solid plus upper o subscript 2 gas right arrow upper C upper O subscript 2 gas Delta H 1 equals negative 393.5 kilojoules. 2: 2 upper C upper O gas plus upper O subscript 2 gas right arrow 2 upper C upper O subscript 2 gas Delta H 2 equals negative 566.0 kilojoules. 3: 2 upper H subscript 2 upper o gas right arrow 2 upper H subscript 2 gas plus upper O subscript 2 gas delta H 3 equals 483.6 kilojoules.

The overall chemical equation is Upper C (s) plus upper H subscript 2 upper O (g) right arrow upper C upper o (g) plus upper H subscript 2 (g).. To calculate the final enthalpy of the overall chemical equation, which step must occur?

~Reverse the first equation, and change the sign of the enthalpy. Then, add.
~Reverse the second equation, and change the sign of the enthalpy. Then, add.
~Multiply the first equation by three, and triple the enthalpy. Then, add.
~Divide the third equation by two, and double the enthalpy. Then, add.

Respuesta :

Answer: The enthalpy of the second intermediate equation is halved and has its sign changed.

Explanation:

Let us take a look at the first and second intermediate reactions as well as the overall reaction equation for the process under review;

First reaction;

Ca (s) + CO₂ (g) + ½O₂ (g) → CaCO₃ (s) ΔH₁ = -812.8 kJ

Second reaction;

2Ca (s) + O₂ (g) → 2CaO (s) ΔH₂ = -1269 kJ

Hence the overall equation is now;

CaO (s) + CO₂ (g) → CaCO₃ (s) ΔH = ?

According to the Hess law of constant heat summation, the enthalpy of the overall reaction is supposed to be obtained as a sum of the enthalpy of both reactions but this will not give the enthalpy of the overall reaction in this case. The enthalpy of the overall reaction is rather obtained by halving the enthalpy of the second intermediate reaction and reversing its sign before taking the sum as shown below;

Enthalpy of Intermediate reaction 1 + ½(- Enthalpy of Intermediate reaction 2) = Enthalpy of Overall reaction

The final enthalpy will be:

The enthalpy of the second intermediate equation is halved and has its sign changed.

Hess's law:

First reaction:

Ca (s) + CO₂ (g) + ½O₂ (g) → CaCO₃ (s) ΔH₁ = -812.8 kJ

Second reaction:

2Ca (s) + O₂ (g) → 2CaO (s) ΔH₂ = -1269 kJ

Overall reaction:

CaO (s) + CO₂ (g) → CaCO₃ (s) ΔH = ?

According to the Hess law of constant heat summation, the enthalpy of the overall reaction is the sum of the enthalpy of both reactions but this will not give the enthalpy of the overall reaction in this case. The enthalpy of the overall reaction is rather obtained by halving the enthalpy of the second intermediate reaction and reversing its sign before taking the sum as shown below;

Enthalpy of Intermediate reaction 1 + ½(- Enthalpy of Intermediate reaction 2) = Enthalpy of Overall reaction

Find more information about Enthaply change here:

brainly.com/question/26991394

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