How much heat is absorbed when 42 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO2(g) –> CS2(l) + 4 CO(g) ΔH° = +239.9 kJ Hint: Convert from mass to moles of C(s) (dividing the mass by the molar mass of C), then multiply by the molar heat of reaction (239.9 kJ / 5 moles C). Group of answer choices178 kJ168 kJ148 kJ158 kJ
Question
How much heat is absorbed when 42 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO2(g) –> CS2(l) + 4 CO(g) ΔH° = +239.9 kJ Hint: Convert from mass to moles of C(s) (dividing the mass by the molar mass of C), then multiply by the molar heat of reaction (239.9 kJ / 5 moles C). Group of answer choices178 kJ168 kJ148 kJ158 kJ
Solution
To solve this problem, we first need to convert the mass of carbon (C) to moles. The molar mass of carbon is approximately 12.01 g/mol.
So, 42 g of C is equivalent to 42 g / 12.01 g/mol = 3.5 moles of C.
The given chemical equation tells us that 5 moles of C react to absorb 239.9 kJ of heat. Therefore, the heat absorbed per mole of C is 239.9 kJ / 5 moles = 47.98 kJ/mol.
Finally, we can find the total heat absorbed when 3.5 moles of C react by multiplying the moles of C by the heat absorbed per mole of C:
3.5 moles * 47.98 kJ/mol = 167.93 kJ
So, the closest answer is 168 kJ.
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