the combustion of one mole of butane proceeds according to the following unbalanced reaction: 1 c₄h₁₀ + o₂ →…
the combustion of one mole of butane proceeds according to the following unbalanced reaction: 1 c₄h₁₀ + o₂ → co₂ + h₂o. what is the coefficient in front of dioxygen when the reaction is properly balanced for one mole of butane? select one: a. 1.5 b. 9 c. 13 d. 8 e. 6.5 clear my choice
Answer
Explanation:
Step1: Balance carbon atoms
For 1 mole of $C_4H_{10}$, to balance the carbon - atoms on the right - hand side, since there are 4 carbon atoms in $C_4H_{10}$, the coefficient of $CO_2$ should be 4. So the reaction becomes $C_4H_{10}+O_2\rightarrow4CO_2 + H_2O$.
Step2: Balance hydrogen atoms
There are 10 hydrogen atoms in $C_4H_{10}$. To balance the hydrogen atoms, the coefficient of $H_2O$ should be 5 (because $2\times5 = 10$). So the reaction is $C_4H_{10}+O_2\rightarrow4CO_2+5H_2O$.
Step3: Balance oxygen atoms
On the right - hand side, the total number of oxygen atoms is $4\times2 + 5\times1=8 + 5=13$. So the coefficient of $O_2$ should be $\frac{13}{2}=6.5$ to balance the oxygen atoms. The balanced reaction is $C_4H_{10}+6.5O_2\rightarrow4CO_2 + 5H_2O$.
Answer:
e. 6.5