Practice Mole Ratios And Reaction Stoichiometry (1.2.2) - Unit 1: Stoichiometric Relationships

Practice: Mole Ratios and Reaction Stoichiometry

Lesson 1.2.2Unit 1: Stoichiometric Relationships

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9 questions

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6 sample questions

Question 1.
What is the mole ratio of O₂ to CO₂ in the equation 2 H₂ + O₂ ⟶ 2 H₂O?
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Check the coefficients of O₂ and H₂O.
Question 2.
If you have 4 moles of H₂, how many moles of O₂ are needed?
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Use the balanced equation to determine the ratio.
3Question 3.
What is the mole ratio of reactant to product in a balanced chemical equation?
- It is arbitrary.
- It means the same as the balanced equation coefficients.
- It has no meaning.
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Refer to the definition of mole ratios.
4Question 4.
True or False: The balanced equation can change depending on the coefficients we use.
- True
- False
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Think about the concept of conservation of mass.
Question 5.
In a combustion reaction, 23 g of ethane (C₂H₆) is burned in excess oxygen. Determine how many grams of CO₂ are produced.
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Start by balancing the equation and finding molar masses.
Question 6.
Ammonia (NH₃) burns in a reaction with oxygen described by the equation 4 NH₃ + 3 O₂ ⟶ 2 N₂ + 6 H₂O. If you start with 15 g of NH₃, how many grams of water will be produced?
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Perform the conversion for NH₃ to moles and use mole ratios to find water.

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