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Chapter 6: Problem 142

To establish a pressure of 2.00 atm in a 2.24 L cylinder containing \(1.60 \mathrm{g} \mathrm{O}_{2}(\mathrm{g})\) at \(0^{\circ} \mathrm{C},\) (a) add \(1.60 \mathrm{g} \mathrm{O}_{2} ;(\mathrm{b})\) add \(0.60 \mathrm{g} \mathrm{He}(\mathrm{g}) ;(\mathrm{c})\) add \(2.00 \mathrm{g} \mathrm{He}(\mathrm{g})\) (d) release \(0.80 \mathrm{g} \mathrm{O}_{2}(\mathrm{g})\)

Short Answer

Expert verified
Each action should be performed as follows: (a) Add 1.60 g of O2. (b) Add 0.694 g of He. (c) Add 2.00 g of He. (d) Release 0.846 g of O2.

Step by step solution

01

Convert temperature to Kelvin

Temperature in the Ideal Gas Law must be in Kelvin. Convert 0 degrees Celsius to Kelvin using the formula K = °C + 273.15. Hence, the temperature is 273.15 K.
02

Calculate number of moles to achieve desired pressure

Rearrange the Ideal Gas Law to solve for n, the number of moles. n=PV/RT. Substitute P=2.00 atm, V=2.24 L, R=0.0821 L.atm/(mol.K) (Ideal Gas Law constant), T=273.15 K into the formula. This gives the required moles of gas.
03

Calculate mass for given substances

The number of moles obtained in step 2 is used to compute the mass of each gas using their molar masses. (a) For O2 the molar mass is 32.00 g/mol and for He it's 4.00 g/mol. (b, c) Compute the masses for 0.60g of He and 2.00g of He. (d) Deduct mass of 0.8g O2 from the initial 1.6g O2.
04

Add or release required amount of each gas

Add or release the required amount of each gas found in step 3 to the cylinder to achieve the pressure of 2.00 atm.

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Most popular questions from this chapter

Which of the following choices represents the molar volume of an ideal gas at \(25^{\circ} \mathrm{C}\) and 1.5 atm? (a) \((298 \times 1.5 / 273) \times 22.4 \mathrm{L} ;\) (b) \(22.4 \mathrm{L}\) (c) \((273 \times 1.5 / 298) \times 22.4 \mathrm{L}\) (d) \([298 /(273 \times 1.5)] \times 22.4 \mathrm{L}\) (e) \([273 /(298 \times 1.5)] \times 22.4 \mathrm{L}\)

How many liters of \(\mathrm{H}_{2}(\mathrm{g})\) at STP are produced per gram of \(\mathrm{Al}(\mathrm{s})\) consumed in the following reaction? \(2 \mathrm{Al}(\mathrm{s})+6 \mathrm{HCl}(\mathrm{aq}) \longrightarrow 2 \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2}(\mathrm{g})\)

A 0.418 g sample of gas has a volume of \(115 \mathrm{mL}\) at \(66.3^{\circ} \mathrm{C}\) and \(743 \mathrm{mm} \mathrm{Hg} .\) What is the molar mass of this gas?

Carbon monoxide, \(\mathrm{CO}\), and hydrogen react according to the equation below. $$3 \mathrm{CO}(\mathrm{g})+7 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow \mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$$ What volume of which reactant gas remains if \(12.0 \mathrm{LCO}(\mathrm{g})\) and \(25.0 \mathrm{L} \mathrm{H}_{2}(\mathrm{g})\) are allowed to react? Assume that the volumes of both gases are measured at the same temperature and pressure.

Explain why the height of the mercury column in a barometer is independent of the diameter of the barometer tube.
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