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- Write a guide to solving a stoichiometry problem with moles.

For example, calculate moles of CO_{2}made when 3.4 moles of butane (C_{4}H_{10}) are burned, using this chemical equation:

2C_{4}H_{10}+ 13O_{2}→ 8CO_{2}+ 10H_{2}O - Write a guide to solving a stoichiometry problem with grams.

For example, calculate grams of O_{2}used up when 125 grams of butane (C_{4}H_{10}) are burned, using this chemical equation:

2C_{4}H_{10}+ 13O_{2}→ 8CO_{2}+ 10H_{2}O - Write a guide to solving a limiting reactant stoichiometry problem with grams.

For example, calculate grams of H_{2}O made when 125 grams of butane (C_{4}H_{10}) are reacted with 550 grams of oxygen (O_{2}), using this chemical equation:

2C_{4}H_{10}+ 13O_{2}→ 8CO_{2}+ 10H_{2}O - Write a guide to solving a limiting reactant stoichiometry problem with grams.

For example, calculate grams of O_{2}left over when 89 grams of butane (C_{4}H_{10}) are reacted with 475 grams of oxygen (O_{2}). Oxygen is the excess reactant in this problem set-up.

2C_{4}H_{10}+ 13O_{2}→ 8CO_{2}+ 10H_{2}O