Question

Consider the following intermediate chemical equations.

3 equations. 1: upper C upper H subscript 4 (g) right arrow upper C (s) plus 2 upper H subscript 2 (g). Delta H 1 equals 74.8 kilojoules. 2: upper C upper C l subscript 4 (g) right arrow upper C (s) plus 2 upper C l subscript 2 (g). Delta H 2 equals 95.7 kilojoules. Upper H subscript 2 (g) plus upper C l subscript 2 (g) right arrow 2 upper H upper C l (g). Delta H subscript 3 equals negative 92.3 kilojoules.

What is the enthalpy of the overall chemical reaction Upper C upper H subscript 4 (g) plus 4 upper C l subscript 2 (g) right arrow upper C upper C l subscript 4 (g) plus 4 upper H upper C l (g).?
-205.7 kJ
-113.4 kJ
-14.3 kJ
78.0 kJ

Answer 1

A: -205.7

Explanation:

Answer 2

A. -205.7 kJ

Explanation:

The overall enthalpy of reaction be calculated when the intermediate steps are present

formed in a multi-step process.