Solution Found!
Answer: A 2.10-L vessel contains 4.65 g of a gas at 1.00
Chapter 5, Problem 47P(choose chapter or problem)
A 2.10-L vessel contains \(4.65 \mathrm{~g}\) of a gas at \(1.00 \mathrm{~atm}\) and \(27.0^{\circ} \mathrm{C}\). (a) Calculate the density of the gas in grams per liter. (b) What is the molar mass of the gas?
Questions & Answers
QUESTION:
A 2.10-L vessel contains \(4.65 \mathrm{~g}\) of a gas at \(1.00 \mathrm{~atm}\) and \(27.0^{\circ} \mathrm{C}\). (a) Calculate the density of the gas in grams per liter. (b) What is the molar mass of the gas?
ANSWER:Step 1 of 2
Given:
\(\begin{aligned}&\mathrm{T}=27.0^{\circ} \mathrm{C}=27+273=300 \mathrm{~K} \\ &\mathrm{~V}=2.10 \mathrm{~L}\end{aligned}\)
Mass of gas \(=4.65 \mathrm{~g}\)
\(\mathrm{P}=1.00 \mathrm{~atm} .\)
(a) Here, we are asked to calculate the density of the gas in grams per liter:
The formula of density is as shown below:
\(\begin{aligned}\text { Density }(\mathrm{d})=& \frac{\operatorname{mass}(\mathrm{m})}{\operatorname{Volume}(\mathrm{V})} \\&=\frac{4.65 \mathrm{~g}}{2.10 \mathrm{~L}} \\&=\mathbf{2 . 2 1 4} \mathbf{g} / \mathrm{L}\end{aligned}\)
Hence, the density of the gas is \(2.214 \mathrm{~L}\)