How much heat is absorbed when 45.00 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?
5 C(s) + 2 SO₂(g) → CS₂(l) + 4 CO(g)
H° = 239.9 kJ

Question

How much heat is absorbed when 45.00 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?
5 C(s) + 2 SO₂(g) → CS₂(l) + 4 CO(g)

How much heat is absorbed when 45.00 g of C(s) reacts in the presence of excess SO<sub>2</sub>(g) to produce CS<sub>2</sub>(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO<sub>2</sub>(g) → CS<sub>2</sub>(l) + 4 CO(g) H° = 239.9 kJ A) 179.8 kJ B) 239.9 kJ C) 898.5 kJ D) 2158 kJ

H° = 239.9 kJ

Quizplus · Accepted Answer

The given chemical equation states that the reaction of 5 moles of carbon produces 239.9 kJ of heat. 
We need to find the amount of heat absorbed when 45.00 g of carbon reacts. 
First, we need to find the number of moles of carbon:
45.00 g C * (1 mol C/12.01 g) = 3.749 mol C
According to the balanced equation, 5 moles of carbon produce 239.9 kJ of heat, so we can set up a proportion:
5 mol C / 239.9 kJ = 3.749 mol C / x
Solving for x, we get:
x = (3.749 mol C * 239.9 kJ) / 5 mol C = 179.8 kJ
Therefore, the answer is A) 179.8 kJ, which is the amount of heat absorbed when 45.00 g of carbon reacts.

How Much Heat Is Absorbed When 45