To determine the amount of heat evolved during the formation of 0.176 kg of CO, we need to follow these steps:
1. Convert the mass of CO to grams:
- The given mass is 0.176 kg. To convert it to grams, we multiply by 1000:
[tex]\[
0.176 \, \text{kg} \times 1000 = 176 \, \text{g}
\][/tex]
2. Calculate the number of moles of CO:
- The molar mass of CO (carbon monoxide) is given as 28.01 g/mol. We use this to convert the grams of CO to moles:
[tex]\[
\text{Number of moles} = \frac{\text{mass in grams}}{\text{molar mass}}
\][/tex]
[tex]\[
\text{Number of moles of CO} = \frac{176 \, \text{g}}{28.01 \, \text{g/mol}} \approx 6.283
\][/tex]
3. Determine the heat evolved:
- The heat of formation of CO is given as -393 kJ/mol. The total heat evolved is obtained by multiplying the number of moles by the heat of formation:
[tex]\[
\text{Heat evolved} = \text{Number of moles} \times \text{Heat of formation}
\][/tex]
[tex]\[
\text{Heat evolved} = 6.283 \, \text{moles} \times (-393 \, \text{kJ/mol}) \approx -2469.4 \, \text{kJ}
\][/tex]
Given the possible answers:
- (A) -13579 J
- (B) -12759 kJ
- (C) -1572.0 kJ
- (D) -1165.5 kJ
The closest answer to -2469.4 kJ is not listed directly among the given options. However, this indicates that the correct answer might require rounding or an adjustment/error in the provided multiple choice question. Should be -2469.4.
Thus, none of the given answer choices precisely match, but the calculation is accurate and results in -2469.4 kJ of heat evolved for the formation of 0.176 kg of CO.
Please double-check the problem statement or options, as the calculated correct answer does not match any given choice exactly.
