C(s) + O₂(g) → CO₂(g) + 400 kJ

C(s) + $\frac{1}{2}{O}_2\left(g\right)\to CO\left(g\right)+100kJ$  

When coal of purity 60% is allowed to burn in presence of insufficient oxygen, 60% of carbon is converted into ‘CO’ and the remaining is converted into ‘CO₂’.

The heat generated when 0.6 kg of coal is burnt is

<p>Mass of pure carbon in coal = 0.6 × 1000gm ×&nbsp;<math><mrow><mfrac><mrow><mn>6</mn><mn>0</mn></mrow><mrow><mn>1</mn><mn>0</mn><mn>0</mn></mrow></mfrac><mo>=</mo><mn>3</mn><mn>6</mn><mn>0</mn><mi>g</mi><mi>m</mi></mrow></math></p><p>Mass of carbon converted into CO = 6&nbsp;<math><mrow><mfrac><mrow><mn>6</mn><mn>0</mn></mrow><mrow><mn>1</mn><mn>0</mn><mn>0</mn></mrow></mfrac><mo>×</mo><mn>3</mn><mn>6</mn><mn>0</mn><mo>=</mo><mn>2</mn><mn>1</mn><mn>6</mn><mi>g</mi><mi>m</mi><mo>⇒</mo><mi>M</mi><mi>o</mi><mi>l</mi><mo>=</mo><mfrac><mrow><mn>2</mn><mn>1</mn><mn>6</mn></mrow><mrow><mn>1</mn><mn>2</mn></mrow></mfrac><mo>=</mo><mn>1</mn><mn>8</mn></mrow></math>&nbsp;mole of carbon</p><p>Mass of carbon converted into CO₂ = 360 – 216 = 144gm Mole =&nbsp;<math><mrow><mfrac><mrow><mn>1</mn><mn>4</mn><mn>4</mn></mrow><mrow><mn>1</mn><mn>2</mn></mrow></mfrac><mo>=</mo><mn>1</mn><mn>2</mn></mrow></math>&nbsp;mole of carbon.</p><p>C (s) + O₂ (g) CO₂ (g) + 400KJ</p><p>Mole – 12 for CO₂ production, Hence total energy produced = 400 × 12 = 4800KJ</p><p><math><mrow><msub><mrow><mi>C</mi></mrow><mrow><mrow><mo> (</mo><mrow><mi>s</mi></mrow><mo>)</mo></mrow></mrow></msub><mo>+</mo><mfrac><mrow><mn>1</mn></mrow><mrow><mn>2</mn></mrow></mfrac><msub><mrow><mi>O</mi></mrow><mrow><mn>2</mn></mrow></msub><mrow><mo> (</mo><mrow><mi>g</mi></mrow><mo>)</mo></mrow><munderover><mo>→</mo><mrow></mrow><mrow></mrow></munderover><mi>C</mi><msub><mrow><mi>O</mi></mrow><mrow><mrow><mo> (</mo><mrow><mi>g</mi></mrow><mo>)</mo></mrow></mrow></msub><mo>+</mo><mn>1</mn><mn>0</mn><mn>0</mn><mi>K</mi><mi>J</mi></mrow></math></p><p>Mole = 18 for CO production, Hence energy produced = 100 × 18 = 1800KJ</p><p>Total heat = 4800 + 1800 = 6600KJ</p>

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