Question

0.5 gm of an organic compound with 60%. Carbon produce ______ gm of \(CO_{2}\) upon complete combustion

Answer 1

Correct Answer: 1.1

The given organic compound contains 60% carbon. To determine the mass of \(CO_{2}\) produced, we follow these steps:

1. Calculate the mass of carbon in the compound:
Mass of carbon = \(0.5\, \text{gm} \times 60\%\) = \(0.3\, \text{gm}\).

2. Use the stoichiometry of the reaction to determine the mass of \(CO_{2}\) produced. The molar mass of carbon is approximately \(12\, \text{g/mol}\), and the molar mass of \(CO_{2}\) is approximately \(44\, \text{g/mol}\).

3. Since carbon in the compound produces \(CO_{2}\), where 1 mol of carbon gives 1 mol of \(CO_{2}\), the mass of \(CO_{2}\) is calculated using the ratio:

Mass of \(CO_{2}\) = \(\frac{44\, \text{g/mol}}{12\, \text{g/mol}} \times 0.3\, \text{gm} = 1.1\, \text{gm}\).

4. Verify the calculated mass falls within the given range (1.1, 1.1). The computed mass \(1.1\, \text{gm}\) matches exactly, confirming the solution is correct.

Therefore, upon complete combustion, \(0.5\, \text{gm}\) of the organic compound produces \(1.1\, \text{gm}\) of \(CO_{2}\).