Answered

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Use the following information to answer the questions below:

[tex]\[
2H_2O(l) \rightarrow 2H_2(g) + O_2(g) \quad \Delta H = 572 \text{ kJ}
\][/tex]

1. This reaction is:
A. endothermic
B. exothermic

2. Suppose [tex]95.2 \, g[/tex] of [tex]H_2O[/tex] react. Will any heat be released or absorbed?
A. Yes, absorbed
B. Yes, released
C. No

3. If you said heat will be released or absorbed in the previous question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits.

[tex]\[
\boxed{\text{ }} \text{ kJ}
\][/tex]

Sagot :

GinnyAnswer
To solve the given questions, let's analyze the given reaction and data step-by-step:

1. Determining the type of reaction:
The given reaction is:
[tex]\[ 2 H_2O(l) \rightarrow 2 H_2(g) + O_2(g) \quad \Delta H = 572 \, \text{kJ} \][/tex]
The change in enthalpy [tex]\(\Delta H\)[/tex] is positive, indicating that the reaction absorbs heat from the surroundings.
Therefore, the reaction is endothermic.

Answer: This reaction is endothermic.

2. Heat absorption or release:
Now, we need to determine if heat will be absorbed or released when 95.2 grams of [tex]\( H_2O \)[/tex] react. Since the reaction is endothermic, it will absorb heat.

Answer: Yes, absorbed.

3. Calculating the amount of heat absorbed:
To calculate how much heat will be absorbed when 95.2 grams of water react, follow these steps:

- Calculate the molar mass of [tex]\( H_2O \)[/tex]:
[tex]\[ \text{Molar mass of } H_2O = 2 \times 1.01\, \text{g/mol} + 16.00\, \text{g/mol} = 18.02\, \text{g/mol} \][/tex]

- Calculate the number of moles of [tex]\( H_2O \)[/tex]:
[tex]\[ \text{moles of } H_2O = \frac{95.2\, \text{g}}{18.02\, \text{g/mol}} \approx 5.283\, \text{moles} \][/tex]

- Determine the heat absorbed:
The given [tex]\(\Delta H\)[/tex] value of 572 kJ corresponds to the reaction of 2 moles of [tex]\( H_2O \)[/tex].
Therefore, the heat absorbed per mole of [tex]\( H_2O \)[/tex] is:
[tex]\[ \frac{572\, \text{kJ}}{2} = 286\, \text{kJ/mol} \][/tex]
For 5.283 moles of [tex]\( H_2O \)[/tex]:
[tex]\[ \text{Heat absorbed} = 286\, \text{kJ/mol} \times 5.283\, \text{moles} \approx 1510.943\, \text{kJ} \][/tex]

Answer: The amount of heat absorbed is 1510.943 kJ.

In summary:
[tex]\[ \boxed{1510.943 \, \text{kJ}} \][/tex]
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