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Exam 3: Equations, the Mole, and Chemical Formulas

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Question 51

Multiple Choice

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What is the mass in grams of 3.0×10¹⁵ atoms of C?

A) 5.0×10 ^{- 9} g
B) 6.0×10 ^{- 8} g
C) 2.4×10⁹ g
D) 3.6×10¹⁶ g
E) none of these

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Question 52

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How many atoms are present in 2.7 g of B?

A) 1.5×10²³
B) 3.0×10²³
C) 8.2×10²²
D) 9.6×10²²
E) none of these

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Question 53

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In the reaction of 16.3 g of C₂H₄O with 10.4 g of O₂, a chemist isolates 2.3 g of H₂0. What is the percent yield?

How many moles of sodium chloride are present in 5.84 grams of NaCl?

Exhibit 3-2 Aluminum sulfide, Al₂S₃ (molar mass = 150.16 g/mol) , reacts with water to form the aluminum hydroxide, Al(OH) ₃ (molar mass = 78.00 g/mol) , and hydrogen sulfide, H₂S, as shown below: __ Al₂S₃ + __ H₂O→__ Al(OH) ₃ + __ H₂S (unbalanced reaction) Refer to Exhibit 3-2. How many grams of aluminum hydroxide, Al(OH) ₃, is obtained from 10.5 g of aluminum sulfide, Al₂S₃?

How many sulfur atoms are present in 10.0 grams of Sulfur?

What is the oxidation number of the manganese atom in the formula for the compound KMnO₄?

What is the empirical formula for a compound that has the following mass percent composition: C, 55.80%; H, 7.03%; O, 37.17%.

What is the molar mass of magnesium phosphate?

What is the molar mass of iron?

If a 0.24 g sample is burned in air to produce 0.22 g CO₂, what is the percent carbon in the sample?

What is the molecular formula for Lactic acid if an elemental analysis of this compound shows that it contains 40.0 mass % C, 6.71 mass % H and 53.3 mass % O and a mass spectrometry experiment indicates its molar mass is 90.08 g/mol.

How many grams of N₂H₄ are produced from the reaction of 2.0 g of H₂ witH₂ 8 g of N₂ as shown in the following balanced equation? 2 H₂ + N₂→N₂H₄

What mass of CO₂ is produced by burning 4.1 g of C₂H₄ in excess O₂?

What is the ratio of A/B for the equation below where A , B , C , and D represent the coefficients in the balanced equation? A C₄H₈O + B O₂→C CO₂ + D H₂O

A 0.100 g sample of a compound containing only C and H is burned in excess oxygen, producing 0.338 g of CO₂ and 0.0692 g of H₂O. What is the empirical formula of the compound?

The equation representing the chemical change used to produce W is shown below. What mass of W is produced from 2.0 g H₂ and 50 g of WO₃? WO₃ + 3 H₂→W + 3 H₂O

How many grams of CO₂ are produced from burning 4.20 g C₂H₄ in air?

What mass of water is produced by burning 4.2 g O₂ in excess H₂?

What is the oxidation number of the cobalt in CoCl₂?