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Here is the problem: In the reaction CH4 plus O2 → CO2 plus H2O, how many grams of CO2 form from 16 g of CH4?

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Balance atoms of every element, then use the coefficients as mole ratios.

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Write an atom balance for each element. Give each species an unknown coefficient; atoms of every element must be equal on both sides.

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Solve the linear system with the smallest whole numbers. Exact elimination leaves one free coefficient; scaling by the least common denominator gives integers.

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Balanced equation.

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Moles of CH4.

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CO2 via the mole ratio 1: 1.

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So the answer is CH4 plus 2O2 → CO2 plus 2H2O; 16 g CH4 → CO2: 43.891 g (0.99732 mol).

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Coefficients in a balanced equation count particles (moles), not grams. Convert grams to moles, apply the mole ratio, then convert back to grams with the other species prime molar mass. Assumes the reaction goes to completion with the known species fully consumed (or formed).

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C: 1 equals 1, H: 4 equals 4, O: 4 equals 4, which checks out.

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CO2 is produced in a 1: 1 mole ratio to CH4.