Question

Use the following data: \[ \begin{array}{ll} \mathrm{H}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) & \Delta \mathrm{H}^{0}=-285.8 \mathrm{~kJ} \\ \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) & \Delta \mathrm{H}^{0}=-187.8 \mathrm{~kJ} \end{array} \] to calculate \( \Delta \mathrm{H}^{0} \) for the decomposition of hydrogen peroxide according to the following equation: \[ 2 \mathrm{H}_{2} \mathrm{O}_{2} \text { (aq) } \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{0}=\text { ??? } \] \( -196.0 \mathrm{~kJ} \) \( -98.0 \mathrm{~kJ} \) \( -89.8 \mathrm{~kJ} \) \( -767.6 \mathrm{~kJ} \) \( -383.8 \mathrm{~kJ} \)

          Use the following data:
\[
\begin{array}{ll}
\mathrm{H}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) & \Delta \mathrm{H}^{0}=-285.8 \mathrm{~kJ} \\
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) & \Delta \mathrm{H}^{0}=-187.8 \mathrm{~kJ}
\end{array}
\]
to calculate \( \Delta \mathrm{H}^{0} \) for the decomposition of hydrogen peroxide according to the following equation:
\[
2 \mathrm{H}_{2} \mathrm{O}_{2} \text { (aq) } \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{0}=\text { ??? }
\]
\( -196.0 \mathrm{~kJ} \)
\( -98.0 \mathrm{~kJ} \)
\( -89.8 \mathrm{~kJ} \)
\( -767.6 \mathrm{~kJ} \)
\( -383.8 \mathrm{~kJ} \)

Use the following data:

H2( g)+1 / 2 O2( g) →H2O(l) ΔH^0=-285.8 kJ
H2( g)+O2( g) →H2O2(aq) ΔH^0=-187.8 kJ

to calculate ΔH^0 for the decomposition of hydrogen peroxide according to the following equation:

2 H2O2 (aq) → 2 H2O(ℓ)+O2( g) ΔH^0= ???

-196.0 kJ
-98.0 kJ
-89.8 kJ
-767.6 kJ
-383.8 kJ

Added by P (.

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