Answered

Welcome to Westonci.ca, where finding answers to your questions is made simple by our community of experts. Connect with a community of professionals ready to provide precise solutions to your questions quickly and accurately. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals.

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]

What is [tex]\(\Delta H_{\text{rxn}}\)[/tex] for the overall reaction?
[tex]\[ \boxed{\text{kJ}} \][/tex]

Sagot :

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

[tex]\[ \text{CH}_4(g) + 2 \text{O}_2(g) \rightarrow \text{CO}_2(g) + 2 \text{H}_2\text{O}(l) \][/tex]

we need to consider the enthalpy changes ([tex]\(\Delta H\)[/tex]) of the two given steps:

1. For the reaction:
[tex]\[ \text{CH}_4(g) + 2 \text{O}_2(g) \rightarrow \text{CO}_2(g) + 2 \text{H}_2\text{O}(g), \quad \Delta H_1 = -802 \, \text{kJ} \][/tex]

2. For the phase change:
[tex]\[ 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{H}_2\text{O}(l), \quad \Delta H_2 = -88 \, \text{kJ} \][/tex]

We can combine these two reactions to find the overall enthalpy change for the conversion of methane and oxygen into carbon dioxide and liquid water.

The overall reaction is formed by summing these two reactions:

[tex]\[ \left( \text{CH}_4(g) + 2 \text{O}_2(g) \rightarrow \text{CO}_2(g) + 2 \text{H}_2\text{O}(g), \quad \Delta H_1 = -802 \, \text{kJ} \right) \][/tex]

[tex]\[ + \][/tex]

[tex]\[ \left( 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{H}_2\text{O}(l), \quad \Delta H_2 = -88 \, \text{kJ} \right) \][/tex]

Thus, the overall reaction is:

[tex]\[ \text{CH}_4(g) + 2 \text{O}_2(g) \rightarrow \text{CO}_2(g) + 2 \text{H}_2\text{O}(l) \][/tex]

To find the overall enthalpy change ([tex]\(\Delta H_{\text{rxn}}\)[/tex]), we add the enthalpy changes of the two steps:

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

Given that:

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

Combining these, we get:

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

Therefore, the enthalpy change ([tex]\(\Delta H_{\text{rxn}}\)[/tex]) for the overall reaction is:

[tex]\[ -890 \, \text{kJ} \][/tex]
Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. Keep exploring Westonci.ca for more insightful answers to your questions. We're here to help.