contestada

How much heat is absorbed when 30.00 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) ΔH° = +239.9 kJ

Respuesta :

maacastrobr

Answer:

120.0 kJ

Explanation:

  • First we convert the given mass of C to moles:

30.00 g C ÷ 12g/mol = 2.5 mol

  • The ΔH° value given by the problem, is the heat absorbed when 5 moles of C react.

So when we have half the moles of C (2.5 instead of 5.0), the heat absorbed will also be half, thus the answer is:

  • 239.9 kJ / 2 = 120.0 kJ

120kJ of heat is absorbed when 30.00 g of C(s) reacts in the presence of excess SO₂(g) to produce CS₂(l) and CO(g).

What is heat enthalpy?

Enthalpy of a reaction is the amount of heat that is released or absorbed during a chemical reaction.

In the question given that,

5C(s) + 2SO₂(g) → CS₂(l) + 4CO(g), ΔH° = +239.9 kJ

From the reaction it is clear that 239.9 kJ amount of heat is released when 5 moles of carbon reacts to form product.

First we convert the given mass of carbon to moles by using formula:

n = W/M, where

W = given mass of carbon = 30g

M= molar mass of carbon 12g/mol

n = 30 / 12 = 2.5 moles.

So, heat absorbed for the 2.5 moles of carbon is half of the heat absorbed by 5 moles of carbon i.e. 239.9 kJ/2 = 120kJ.

Hence, 120kJ of heat is absorbed when 30 g of carbon reacts.

To learn more about heat enthalpy, visit below link:

https://brainly.com/question/13439286

Otras preguntas