determine the mass in grams of c4h10 that are required to completely react to produce 8.70 mol of co2…

determine the mass in grams of c4h10 that are required to completely react to produce 8.70 mol of co2 according to the following combustion reaction: 2 c4h10(g) + 13 o2(g) → 8 co2(g) + 10 h2o(g)

determine the mass in grams of c4h10 that are required to completely react to produce 8.70 mol of co2 according to the following combustion reaction: 2 c4h10(g) + 13 o2(g) → 8 co2(g) + 10 h2o(g)

Answer

Answer:

$31.9$

Explanation:

Step1: Determine mole - ratio

From the balanced equation $2C_4H_{10}(g)+13O_2(g)\rightarrow8CO_2(g) + 10H_2O(g)$, the mole - ratio of $C_4H_{10}$ to $CO_2$ is $\frac{n_{C_4H_{10}}}{n_{CO_2}}=\frac{2}{8}=\frac{1}{4}$.

Step2: Calculate moles of $C_4H_{10}$

Given $n_{CO_2}=8.70$ mol. Using the mole - ratio, $n_{C_4H_{10}}=\frac{1}{4}\times n_{CO_2}=\frac{1}{4}\times8.70$ mol $ = 2.175$ mol.

Step3: Calculate molar mass of $C_4H_{10}$

The molar mass of $C_4H_{10}$, $M=(4\times12.01 + 10\times1.01)$ g/mol$=(48.04+10.1)$ g/mol $= 58.14$ g/mol.

Step4: Calculate mass of $C_4H_{10}$

Using the formula $m = n\times M$, where $n = 2.175$ mol and $M = 58.14$ g/mol. So $m=2.175$ mol$\times58.14$ g/mol$\approx31.9$ g.