How much heat is absorbed when 50.00 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? 5C(s)+ 2SO₂(g)? CS₂(l)+ 4CO(g) $\Delta _ { \mathrm { r } }$ H° = 239.9 kJ

Question

Quizplus · Accepted Answer

First, we need to find the amount of moles of C(s) used in the reaction. 
Molar mass of C(s) = 12.01 g/mol 
n(C) = 50.00 g/12.01 g/mol = 4.165 mol

According to the balanced chemical equation, the reaction produces 239.9 kJ of heat per 5 moles of C(s) reacted. 
So, for 4.165 mol of C(s) reacted, the heat absorbed can be calculated as: 
Heat absorbed = (4.165 mol / 5 mol) x 239.9 kJ 
Heat absorbed = 199.7 kJ/mol

Therefore, the answer is A) 199.7 kJ/mol.

How Much Heat Is Absorbed When 50 Δr\Delta _ { \mathrm { r } }Δr​

How Much Heat Is Absorbed When 50 $\Delta _ { \mathrm { r } }$