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-' a 0 wrting answe 81%)-. Wed 8:12 PM + app.tophat.com Lecture 1-Int. Top Hat Chat with Top Contact Main chemistry syr.... 39%) CH10: Gases Fullscreen Export PDF Problem Statement: A 5.00 LN2 gas sample at a pressure of 1.20 atm and temperature of 15.8°C has a mass of 7.08 g. What is the mass of a 10.0 L H2 gas sample at the same temperature and pressure as the N2 gas sample? Strategy: Because the substances used in this question are gases, Avogadro's law applies Notice that because temperature and pressure are held constant the N2 and H2 sample volumes are proportional to the number of moles. Let's use these facts to solve the problem. Step 1: From the N2 sample mass we can determine moles of N2 Assigned as Homework Q10.24a How many moles of N2 gas are in the sample? Numeric Answer

Explanation / Answer

Moles of N2 = mass/molecular weight

= 7.08 g / 28g/mol

= 0.2528 mol

From the Avogadro law at constant temperature and pressure

Volume of N2 / Volume of H2 = moles of N2 / moles of H2

5L / 10L = (0.2528 mol) / Moles of H2

0.5 = (0.2528 mol) / (moles of H2)

moles of H2 = 0.5057 mol

Mass of H2 gas = moles x molecular weight

= 0.5057 mol x 2 g/mol

= 1.011 g

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