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N2(g) + 3H2(g) → 2NH3(g)ΔH = -92.2 kJ H2(g) + Cl2(g) → 2HCl(g)ΔH = -184.7 kJ N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s)ΔH = -628.9 kJ Find the ΔH of the following reaction:    NH3(g) + HCl(g) → NH4Cl(s)

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N2(g) + 3H2(g) → 2NH3(g)ΔH = -92.2 kJH2(g) + Cl2(g) → 2HCl(g)ΔH = -184.7 kJN2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s)ΔH = -628.9 kJFind the ΔH of the following reaction:NH3(g) + HCl(g) → NH4Cl(s)

Hess&rsquo;s law states that the total enthalpy change of a reaction remains same whether the reaction occurs in one step or in a number of steps.According to Hess&rsquo;s law,<ol><li>The enthalpy change of a reaction becomes half, if its coefficients are divided by 2.</li><li>The sign of enthalpy change gets reversed on reversing the chemical reaction.</li><li>The enthalpy change of a reaction becomes twice, if its coefficients are multiplied with 2.</li></ol>

Reverse the first reaction and divide it by 2.

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N2(g) + 3H2(g) → 2NH3(g)ΔH = -92.2 kJ
H2(g) + Cl2(g) → 2HCl(g)ΔH = -184.7 kJ
N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s)ΔH = -628.9 kJ
Find the ΔH of the following reaction:
<table>
<tbody>
<tr>
<td>NH3(g) + HCl(g) → NH4Cl(s)</td>
</tr>
</tbody>
</table>

N2(g) + 3H2(g) → 2NH3(g)ΔH = -92.2 kJ H2(g) + Cl2(g) → 2HCl(g)ΔH = -184.7 kJ N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(s)ΔH = -628.9 kJ Find the ΔH of the following reaction: NH3(g) + HCl(g) → NH4Cl(s)

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