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Chapter 6: Problem 141

At \(0^{\circ} \mathrm{C}\) and 0.500 atm, 4.48 L of gaseous \(\mathrm{NH}_{3}\) (a) contains \(6.02 \times 10^{22}\) molecules; (b) has a mass of \(17.0 \mathrm{g} ;(\mathrm{c})\) contains \(0.200 \mathrm{mol} \mathrm{NH}_{3} ;\) (d) has a mass of \(3.40 \mathrm{g}\).

Short Answer

Expert verified
The answers are: (a) 0.1 mol, (b) 0.998 mol, (c) 0.200 mol, (d) 0.200 mol.

Step by step solution

01

Calculations for part (a)

We know that at \(0^{\circ} \mathrm{C}\) and 0.500 atm, 4.48 L of gaseous NH_3 contains \(6.02 \times 10^{22}\) molecules. Since \(6.02 \times 10^{23}\) molecules form a mole, thus \(6.02 \times 10^{22}\) molecules will form \(6.02 \times 10^{22} / 6.02 \times 10^{23} = 0.1\) mole of NH_3.
02

Calculations for part (b)

The molar mass of NH_3 is 14.007 (Nitrogen) + 3*1.008 (Hydrogen) = 17.031 g/mol. So, 17.0 g of NH_3 is equal to \(17.0 g / 17.031 g/mol = 0.998\) moles.
03

Answer for part (c)

As no calculations are required here, we just state that under the conditions given, 4.48 L of gaseous NH_3 contains 0.200 mol.
04

Calculations for part (d)

Since the molar mass of NH_3 is 17.031 g/mol, thus 3.40 g of NH_3 is equal to \(3.40 g / 17.031 g/mol = 0.200\) moles.

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Most popular questions from this chapter

A nitrogen molecule ( \(\mathrm{N}_{2}\) ) having the average kinetic energy at \(300 \mathrm{K}\) is released from Earth's surface to travel upward. If the molecule could move upward without colliding with other molecules, then how high would it go before coming to rest? Give your answer in kilometers. [Hint: When the molecule comes to rest, the potential energy of the molecule will be \(m g h\) where \(m\) is the molecular mass in kilograms, \(g=9.81 \mathrm{m} \mathrm{s}^{-2}\) is the acceleration due to gravity, and \(h\) is the height, in meters, above Earth's surface.]

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.

\(\mathrm{Kr}(\mathrm{g})\) in a 18.5 L cylinder exerts a pressure of \(11.2 \mathrm{atm}\) at \(28.2^{\circ} \mathrm{C} .\) How many grams of gas are present?

At times, a pressure is stated in units of mass per unit area rather than force per unit area. Express \(P=1 \mathrm{atm}\) in the unit \(\mathrm{kg} / \mathrm{cm}^{2}\) [Hint: How is a mass in kilograms related to a force?]

What is the mass of argon gas in a \(75.0 \mathrm{mL}\) volume at STP?
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