Question

C3H7OH + O2 -> CO2 + H20balance the equation then find mole ratio of oxygen to water, how many mores of carbon dioxide are produced when 4.6 mol of oxygen react, and how many molecules of C3H7OH will react with 4.6 L of O2?

Answer 1

mole ratio = 9:8

moles of CO2 = 3.07moles

molecules of C3H7OH = 2.75 * 10^22 molecules

Explanations

The balanced form of the chemical rreaction is as shown below;

`2C_3H_7OH+9O_2\rightarrow6CO_2+8H_2O`

The mole ratio of oxygen to water as shown in the equation is 9:8

Given the following parameter

mole of oxygen that reacted = 4.6moles

According to stoichiometry, 9moles of oxygen produces 6 moles of caron dioxide. The moles of CO2 that is required will be expressed as:

`\begin{gathered} moles\text{ of CO}_2=(6)/(9)*4.6moles\text{ of O}_2 \\ moles\text{ of CO}_2=3.07moles \end{gathered}`

Hence the moles of CO2 that will be produced is 3.07moles

Also if 4.6L of O2 reacted, the moles of oxygen that reacted will be;

`\begin{gathered} moles\text{ of O}_2=(4.6)/(22.4)(1mole\text{ = 22.4L}) \\ moles\text{ of O}_2=0.205moles \end{gathered}`

According to stochiometry, 2 moles of C3H7OH reacts with 9moles of oxygen, the moles of C3H7OH required will be:

`\begin{gathered} moles\text{ of C}_3H_7OH=(2)/(9)*0.205 \\ moles\text{ of C}_3H_7OH=0.0456moles \end{gathered}`

Convert the moles of C3H7OH to molecules as shown

`\begin{gathered} molecules\text{ of }C_3H_7OH=0.0456*6.02*10^(23) \\ molecules\text{ of }C_3H_7OH=0.275*10^(23) \\ molecules\text{ of }C_3H_7OH=2.75*10^(22)molecules \end{gathered}`