how many liters of co₂ form from 28 g c₂h₄ and excess o₂ at 1.0 atm and 25 °c?\n$\\ce{c_{2}h_{4} + 3o_{2} ->…

how many liters of co₂ form from 28 g c₂h₄ and excess o₂ at 1.0 atm and 25 °c?\n$\\ce{c_{2}h_{4} + 3o_{2} -> 2co_{2} + 2h_{2}o}$\nvolume of co₂ = ? l\ndo not round until the end.

how many liters of co₂ form from 28 g c₂h₄ and excess o₂ at 1.0 atm and 25 °c?\n$\\ce{c_{2}h_{4} + 3o_{2} -> 2co_{2} + 2h_{2}o}$\nvolume of co₂ = ? l\ndo not round until the end.

Answer

planation:

Step1: Calculate moles of $\text{C}_2\text{H}_4$

Molar mass of $\text{C}_2\text{H}_4$ = $2\times12 + 4\times1 = 28$ g/mol. Moles of $\text{C}_2\text{H}_4$ = $\frac{\text{Mass}}{\text{Molar Mass}} = \frac{28\ \text{g}}{28\ \text{g/mol}} = 1\ \text{mol}$

Step2: Relate moles to $\text{CO}_2$

From reaction: 1 mol $\text{C}_2\text{H}_4$ → 2 mol $\text{CO}_2$. Moles of $\text{CO}_2$ = $1\ \text{mol} \times 2 = 2\ \text{mol}$

Step3: Use ideal gas law for volume

Ideal gas law: $V = \frac{nRT}{P}$ $R = 0.0821\ \frac{\text{L·atm}}{\text{mol·K}}$, $T = 25 + 273 = 298\ \text{K}$, $P = 1.0\ \text{atm}$, $n=2\ \text{mol}$ $V = \frac{2\ \text{mol} \times 0.0821\ \frac{\text{L·atm}}{\text{mol·K}} \times 298\ \text{K}}{1.0\ \text{atm}}$

Step4: Compute final volume

$V = 2 \times 0.0821 \times 298 = 48.9316\ \text{L}$

Answer:

48.93 L (or 49 L if rounded to two significant figures, but following "do not round until end" gives 48.93 L)