To calculate the ΔHrxn for the reaction, we can use Hess's Law, which states that the enthalpy change of a reaction is the sum of the enthalpy changes of the individual steps.

Given the reactions:

1) CaO(s) + 1/2 O2(g) → CaCO3(s) ΔH = -635.1 kJ
2) CaCO3(s) → CaO(s) + CO2(g) ΔH = 178.3 kJ

We want to find the ΔH for the reaction:

3) Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s)

To get this, we need to reverse the second reaction and add it to the first. When we reverse a reaction, we change the sign of ΔH. So the ΔH for the reversed second reaction is -178.3 kJ.

Adding the ΔH values for the first reaction and the reversed second reaction gives us the ΔH for the reaction we're interested in:

ΔHrxn = ΔH1 + ΔH2(reversed) = -635.1 kJ - 178.3 kJ = -813.4 kJ

So, the ΔHrxn for the reaction Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s) is -813.4 kJ.

Question

To calculate the ΔHrxn for the reaction, we can use Hess's Law, which states that the enthalpy change of a reaction is the sum of the enthalpy changes of the individual steps.

Given the reactions:

1) CaO(s) + 1/2 O2(g) → CaCO3(s) ΔH = -635.1 kJ
2) CaCO3(s) → CaO(s) + CO2(g) ΔH = 178.3 kJ

We want to find the ΔH for the reaction:

3) Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s)

To get this, we need to reverse the second reaction and add it to the first. When we reverse a reaction, we change the sign of ΔH. So the ΔH for the reversed second reaction is -178.3 kJ.

Adding the ΔH values for the first reaction and the reversed second reaction gives us the ΔH for the reaction we're interested in:

ΔHrxn = ΔH1 + ΔH2(reversed) = -635.1 kJ - 178.3 kJ = -813.4 kJ

So, the ΔHrxn for the reaction Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s) is -813.4 kJ.

Knowee AI · Accepted Answer

To calculate the ΔHrxn for the reaction, we can use Hess's Law, which states that the enthalpy change of a reaction is the sum of the enthalpy changes of the individual steps.

Given the reactions:

1) CaO(s) + 1/2 O2(g) → CaCO3(s) ΔH = -635.1 kJ
2) CaCO3(s) → CaO(s) + CO2(g) ΔH = 178.3 kJ

We want to find the ΔH for the reaction:

3) Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s)

To get this, we need to reverse the second reaction and add it to the first. When we reverse a reaction, we change the sign of ΔH. So the ΔH for the reversed second reaction is -178.3 kJ.

Adding the ΔH values for the first reaction and the reversed second reaction gives us the ΔH for the reaction we're interested in:

ΔHrxn = ΔH1 + ΔH2(reversed) = -635.1 kJ - 178.3 kJ = -813.4 kJ

So, the ΔHrxn for the reaction Ca(s) + 1/2 O2(g) → CO2(g) + CaCO3(s) is -813.4 kJ.

Calculate ΔHrxn for→+Cas+12O2g CO2g CaCO3sgiven the following set of reactions:→CaOs + Cas12O2g =ΔH635.1kJ→CaCO3s + CaOs CO2g =ΔH178.3kJBe sure your answer has the correct number of significant figures.

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