Explanation Given: Volume of N 2 gas, V N 2 = 58.5 mL Temperature at STP, T = 273 K Pressure at STP, P = 1.0 atm Explanation: Convert the volume of N 2 gas from 58.5 m L to liters by the use of following relation: 1 000 mL = 1 L ∴ 58 .5 mL = 1 L × 58 .5 mL 1000 mL = 0.0585 L The volume occupied by 1 mol of a gas at STP is 22.4L. Use this molar volume to convert the given volume of N 2 gas into their moles. At STP, 22 .4 L of volume is occupied by 1 mol of a gas ∴ 0 .0585 L of volume is occupied by = 1 mol of N 2 gas × 0 .0585 L 22 .4 L = 0.00261 mol of N 2 gas Therefore, 0.00261 mol of N 2 gas occupies 0 .0585 L of volume. Use this number of moles of N 2 to convert into moles of Li by the use of stoichiometric relationships. The given reaction is 6 L i ( s ) + N 2 ( g ) → 2 L i 3 N ( s ) As per the above reaction 1 mol of N 2 gas reacts with 6 mol of Li ∴ 0

Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

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Chapter 5, Problem 76E

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To determine: Mass of lithium that completely reacts with N₂ gas.

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Chapter 5, Problem 75E

Chapter 5, Problem 77E

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Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

Ch. 5 - Prob. 1SAQ Ch. 5 - Prob. 2SAQ Ch. 5 - Prob. 3SAQ Ch. 5 - Prob. 4SAQ Ch. 5 - Prob. 5SAQ Ch. 5 - Prob. 6SAQ Ch. 5 - Prob. 7SAQ Ch. 5 - Prob. 8SAQ Ch. 5 - Q9. A gas sample at STP contains 1.15 g oxygen and...Ch. 5 - Prob. 10SAQ

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