Questions: Question 19 0 pts Refer to the reaction: C2H4 + 3 O2 -> 2 CO2 + 2 H2O How many moles of oxygen are required for the complete reaction of 45 g of C2H4? 4.8 0.64 1.3 x 10^2 8.0 112.5

Question 19
0 pts

Refer to the reaction:
C2H4 + 3 O2 -> 2 CO2 + 2 H2O

How many moles of oxygen are required for the complete reaction of 45 g of C2H4?
4.8
0.64
1.3 x 10^2
8.0
112.5

Transcript text: Question 19 0 pts Refer to the reaction: \[ \mathrm{C}_{2} \mathrm{H}_{4}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \] How many moles of oxygen are required for the complete reaction of 45 g of $\mathrm{C}_{2} \mathrm{H}_{4}$ ? 4.8 0.64 $1.3 \times 10^{2}$ 8.0 112.5

Solution

Solution Steps

Step 1: Determine the Molar Mass of $\mathrm{C}_{2}\mathrm{H}_{4}$

The molar mass of $\mathrm{C}_{2}\mathrm{H}_{4}$ (ethylene) is calculated as follows:

Carbon ($\mathrm{C}$): $2 \times 12.01 \, \text{g/mol} = 24.02 \, \text{g/mol}$
Hydrogen ($\mathrm{H}$): $4 \times 1.008 \, \text{g/mol} = 4.032 \, \text{g/mol}$

Thus, the molar mass of $\mathrm{C}_{2}\mathrm{H}_{4}$ is: \[ 24.02 \, \text{g/mol} + 4.032 \, \text{g/mol} = 28.052 \, \text{g/mol} \]

Step 2: Calculate Moles of $\mathrm{C}_{2}\mathrm{H}_{4}$

To find the number of moles of $\mathrm{C}_{2}\mathrm{H}_{4}$ in 45 g: \[ \text{Moles of } \mathrm{C}_{2}\mathrm{H}_{4} = \frac{45 \, \text{g}}{28.052 \, \text{g/mol}} \approx 1.604 \, \text{mol} \]

Step 3: Use Stoichiometry to Find Moles of $\mathrm{O}_{2}$

From the balanced chemical equation: \[ \mathrm{C}_{2}\mathrm{H}_{4} + 3 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2} + 2 \mathrm{H}_{2}\mathrm{O} \] 1 mole of $\mathrm{C}_{2}\mathrm{H}_{4}$ requires 3 moles of $\mathrm{O}_{2}$.

Thus, 1.604 moles of $\mathrm{C}_{2}\mathrm{H}_{4}$ will require: \[ 1.604 \, \text{mol} \times 3 = 4.812 \, \text{mol of } \mathrm{O}_{2} \]