balance the following reaction and then use it to answer the questions below:\nch₄ + o₂ → h₂o +…

balance the following reaction and then use it to answer the questions below:\n____ch₄ + ____o₂ → ____h₂o + ____co₂\nwhat is the mole ratio of ch₄ to h₂o?\nwhat is the mole ratio of o₂ to co₂?\nhow many moles of h₂o would be produced from 10.5 moles ch₄?\nhow many moles of o₂ would be needed to produce 34.5 moles co₂?

Answer

Answer:

Balance the equation: $CH_4 + 2O_2\rightarrow 2H_2O+CO_2$
Mole - ratio of $CH_4$ to $H_2O$: 1:2
Mole - ratio of $O_2$ to $CO_2$: 2:1
Moles of $H_2O$ from 10.5 moles $CH_4$: 21 moles
Moles of $O_2$ to produce 34.5 moles $CO_2$: 69 moles

Explanation:

Step1: Balance the chemical equation

For carbon, there is 1 carbon in $CH_4$ and 1 in $CO_2$, so the coefficient of $CO_2$ is 1. For hydrogen, there are 4 hydrogens in $CH_4$ and 2 in $H_2O$, so the coefficient of $H_2O$ is 2. For oxygen, there are 2 oxygen atoms in $O_2$ and a total of 4 oxygen atoms on the product - side (2 in $2H_2O$ and 2 in $CO_2$), so the coefficient of $O_2$ is 2. The balanced equation is $CH_4 + 2O_2\rightarrow 2H_2O+CO_2$.

Step2: Determine mole - ratios

From the balanced equation, the mole - ratio of $CH_4$ to $H_2O$ is 1:2 (the coefficients of $CH_4$ and $H_2O$ respectively). The mole - ratio of $O_2$ to $CO_2$ is 2:1 (the coefficients of $O_2$ and $CO_2$ respectively).

Step3: Calculate moles of $H_2O$ from $CH_4$

The mole - ratio of $CH_4$ to $H_2O$ is 1:2. If we have 10.5 moles of $CH_4$, using the proportion $\frac{n_{H_2O}}{n_{CH_4}}=\frac{2}{1}$, then $n_{H_2O}=2\times n_{CH_4}=2\times10.5 = 21$ moles.

Step4: Calculate moles of $O_2$ from $CO_2$

The mole - ratio of $O_2$ to $CO_2$ is 2:1. If we want to produce 34.5 moles of $CO_2$, using the proportion $\frac{n_{O_2}}{n_{CO_2}}=\frac{2}{1}$, then $n_{O_2}=2\times n_{CO_2}=2\times34.5 = 69$ moles.

balance the following reaction and then use it to answer the questions below:\n____ch₄ + ____o₂ → ____h₂o +…