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Ch.5 - Gases
All textbooksTro 4th EditionCh.5 - GasesProblem 127
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Chapter 5, Problem 127

When 0.583 g of neon is added to an 800 cm³ bulb containing a sample of argon, the total pressure of the gases is 1.17 atm at a temperature of 295 K. Find the mass of the argon in the bulb.

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1
Use the ideal gas law, PV = nRT, to find the number of moles of neon. First, convert the mass of neon to moles using its molar mass (20.18 g/mol).
Calculate the number of moles of neon: n_{Ne} = \frac{0.583 \text{ g}}{20.18 \text{ g/mol}}.
Convert the volume from cm³ to liters: 800 \text{ cm}^3 = 0.800 \text{ L}.
Use the ideal gas law to find the total number of moles of gas in the bulb: n_{total} = \frac{PV}{RT}, where P = 1.17 \text{ atm}, V = 0.800 \text{ L}, R = 0.0821 \text{ L atm/mol K}, and T = 295 \text{ K}.
Subtract the moles of neon from the total moles to find the moles of argon: n_{Ar} = n_{total} - n_{Ne}. Convert the moles of argon to mass using its molar mass (39.95 g/mol).
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