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Question: Two reactions are given below: \[C_{(graphite)} + O_{2(g)} \rightarrow CO_{2(g)};\Delta H = - 393.7...

Two reactions are given below:

C(graphite)+O2(g)→CO2(g);ΔH=−393.7kJ;C_{(graphite)} + O_{2(g)} \rightarrow CO_{2(g)};\Delta H = - 393.7kJ;

C(diamond)→C(graphite);ΔH=−2.1kJC_{(diamond)} \rightarrow C_{(graphite)};\Delta H = - 2.1kJ

What quantity of diamond will give 800 kJ of heat on burning?

A

24.25g24.25g

B

15.24g15.24g

C

2 g

D

12.12g12.12g

Answer

24.25g24.25g

Explanation

Solution

: C(diamond)+O2(g)→CO2(g)C_{(diamond)} + O_{2(g)} \rightarrow CO_{2(g)}

=−393.7+(−2.1)=−395.8kJ= - 393.7 + ( - 2.1) = - 395.8kJ

12 g diamond , gives 395.8kJ.395.8kJ.

800 kJ will be given by,12395.8×800=24.25g\frac{12}{395.8} \times 800 = 24.25g