Cycle 2 Day 2

Multiple Choice

Which of the following reactions is best classified as a double displacement reaction?

Multiple Choice

Identify the type of reaction occurring in the following equation:

• Combination Reaction

• Single Displacement Reaction

• Decomposition Reaction

• Combustion Reaction

Draw

Write the balanced chemical reaction:

Multiple Choice

How many significant figures are in the number 0.00560?

• 2

• 3

• 4

• 5

Multiple Choice

What is the result of 4.56 × 1.4 rounded to the correct number of significant figures?

• 6.384

• 6.38

• 6.4

• 6

Multiple Choice

Calculate and round to the correct number of significant figures:

(3.12 × 4.5) + 0.678

• 14.718

• 15

• 14.72

• 14.7

​Calculate the molar mass of ethane (CH₃CH₃)

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Calculate the molar mass of:

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Calculate the molar mass of:

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Calculate the molar mass of:

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Solve.

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Solve.

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Solve.

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Determine the percent composition of oxygen in carbon dioxide (CO₂).

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A sample of calcium phosphate, Ca₃(PO₄)₂, has a molar mass of 310.2 g/mol.

Calculate the percent composition of phosphorus (P) and Calcium (Ca).

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A hydrated sample of magnesium sulfate, MgSO₄ ⋅ 7H₂O, has a molar mass of 246.5 g/mol. Calculate the percent composition of water in the hydrated compound.

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A compound is found to contain 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. Determine the empirical formula of the compound.

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A sample of a compound contains 4.2 g of nitrogen and 12.0 g of oxygen. Determine the empirical formula of the compound.

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A compound has an empirical formula of CH₂ and a molar mass of 56.0 g/mol. Determine the molecular formula of the compound.

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A compound contains 92.3% carbon and 7.7% hydrogen by mass. The molar mass of the compound is 78.0 g/mol. Determine the molecular formula of the compound.

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A compound is composed of 16.0 g of carbon, 2.0 g of hydrogen, and 32.0 g of oxygen.
a. Determine the empirical formula.
b. If the molar mass of the compound is 180.0 g/mol, what is the molecular formula?

Draw

A compound consists of 54.5% carbon, 9.2% hydrogen, and 36.3% oxygen by mass.
a. Determine the empirical formula.

b. If the molar mass of the compound is 138.0 g/mol, what is the molecular formula?

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A hydrocarbon is burned in excess oxygen, producing 88.0 g of carbon dioxide (CO₂) and 18.0 g of water (H₂O).

a. Determine the empirical formula.

b. If the molar mass of the compound is 30.0 g/mol, what is the molecular formula?

​​A chemistry student determined the empirical formula for titanium sulfide (Ti_xS_y). To do so, she reacted titanium with excess sulfur in a crucible, and recorded the following data:

• Weight of crucible - 11.120 g

• Weight of titanium - 8.820 g

• Weight of crucible and product - 31.700g

What is the empirical formula of titanium suflide?