Question

1. $2c_{2}h_{6} + 7o_{2} \

ightarrow 4co_{2} + 6h_{2}o$
a. how many grams of carbon dioxide are produced for each 8 moles of water produced?
grams a → moles a → moles b → grams b

Explanation:

Step1: Find mole ratio of $CO_2$ to $H_2O$

From the balanced equation: $\frac{n_{CO_2}}{n_{H_2O}} = \frac{4}{6} = \frac{2}{3}$

Step2: Calculate moles of $CO_2$

Given $n_{H_2O}=8\ mol$, solve for $n_{CO_2}$:
$n_{CO_2} = n_{H_2O} \times \frac{2}{3} = 8 \times \frac{2}{3} = \frac{16}{3}\ mol$

Step3: Calculate molar mass of $CO_2$

Molar mass of $C=12.01\ g/mol$, $O=16.00\ g/mol$:
$M_{CO_2} = 12.01 + 2\times16.00 = 44.01\ g/mol$

Step4: Convert moles to grams of $CO_2$

$m_{CO_2} = n_{CO_2} \times M_{CO_2}$
$m_{CO_2} = \frac{16}{3} \times 44.01 = 234.72\ g$

Answer:

234.72 grams of carbon dioxide are produced.