Practice Chapter Summary (1.6) - Unit 1: Stoichiometric Relationships

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6 sample questions

Question 1.
What is the molar mass of water (H₂O)?
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Add the atomic masses of H and O.
Question 2.
How many grams is 0.25 moles of sodium (Na) if the molar mass is 22.99 g/mol?
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Use the formula: mass = moles x molar mass.
3Question 3.
What does 1 mole of any substance represent?
- 6.022 x 10²³ particles
- 1 gram
- 12 grams of carbon
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Think of how we use moles to count atoms and molecules.
4Question 4.
True or False: A balanced chemical equation has equal numbers of atoms for each element on both sides.
- True
- False
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Consider the definition of a balanced equation.
Question 5.
If you react 5.00 g of aluminum with excess chlorine gas to produce aluminum chloride, what is the theoretical yield of AlCl₃?
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Start by finding the moles of Al and use the balanced equation to find moles of AlCl₃ produced.
Question 6.
A solution is prepared by dissolving 58.44 g of NaCl in 500 mL of water. What is its molarity?
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Remember the formula: Molarity = moles of solute / liters of solution.

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