Answered

Get reliable answers to your questions at Westonci.ca, where our knowledgeable community is always ready to help. Our platform connects you with professionals ready to provide precise answers to all your questions in various areas of expertise. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.

Consider the chemical equations shown here:

[tex]\[
\begin{array}{l}
CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) \quad \Delta H_1 = -802 \, \text{kJ} \\
2H_2O(g) \rightarrow 2H_2O(l) \quad \Delta H_2 = -88 \, \text{kJ}
\end{array}
\][/tex]

Which equation shows how to calculate [tex]\(\Delta H_{\text{rxn}}\)[/tex] for the equation below?

[tex]\[
CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)
\][/tex]

Sagot :

GinnyAnswer
To calculate the enthalpy change, [tex]\( \Delta H_{\text{rxn}} \)[/tex], for the reaction:

[tex]\[ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O (l), \][/tex]

we need to combine the enthalpy changes of the given reactions. Here are the two reactions provided:

1. [tex]\( CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g) \)[/tex], with [tex]\( \Delta H_1 = -802 \text{ kJ} \)[/tex]
2. [tex]\( 2 H_2O(g) \rightarrow 2 H_2O(l) \)[/tex], with [tex]\( \Delta H_2 = -88 \text{ kJ} \)[/tex]

The first reaction represents the combustion of methane yielding carbon dioxide and water in the gaseous state. The second reaction represents the phase change of water from gas to liquid.

To find the overall [tex]\( \Delta H_{\text{rxn}} \)[/tex] for the formation of liquid water directly from the combustion of methane, we sum the enthalpy changes of the individual steps:

[tex]\[ \Delta H_{\text{rxn}} = \Delta H_1 + \Delta H_2 \][/tex]

Given the values:

[tex]\[ \Delta H_1 = -802 \text{ kJ} \][/tex]
[tex]\[ \Delta H_2 = -88 \text{ kJ} \][/tex]

Add these together:

[tex]\[ \Delta H_{\text{rxn}} = -802 \text{ kJ} + -88 \text{ kJ} \][/tex]
[tex]\[ \Delta H_{\text{rxn}} = -890 \text{ kJ} \][/tex]

Thus, the equation to calculate [tex]\( \Delta H_{\text{rxn}} \)[/tex] for the reaction:

[tex]\[ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O (l) \][/tex]

is:

[tex]\[ \Delta H_{\text{rxn}} = \Delta H_1 + \Delta H_2 = -802 \text{ kJ} + -88 \text{ kJ} = -890 \text{ kJ} \][/tex]
Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Get the answers you need at Westonci.ca. Stay informed by returning for our latest expert advice.