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Chapter 10: Problem 20

Perform the following conversions: \((\mathbf{a})\) 0.912 atm to torr, \((\mathbf{b})\) 0.685 bar to kilopascals, \((\mathbf{c})\) 655 \(\mathrm{mm}\) Hg to atmospheres, \((\mathbf{d})\) \(1.323 \times 10^{5}\) Pa to atmospheres, \((\mathbf{e})\) 2.50 atm to psi.

Short Answer

Expert verified
The short answer for the conversions is as follows: a) \(0.912\ \text{atm} = 693.12\ \text{Torr}\) b) \(0.685\ \text{bar} = 68.5\ \text{kPa}\) c) \(655\ \text{mm}\ \text{Hg} = 0.8618\ \text{atm}\) d) \(1.323 \times 10^{5}\ \text{Pa} = 1.306\ \text{atm}\) e) \(2.50\ \text{atm} = 36.74\ \text{psi}\)

Step by step solution

01

a) Convert 0.912 atm to Torr

To convert 0.912 atm to Torr, we'll use the conversion factor 1 atm = 760 Torr: \(0.912\ \text{atm}\times \dfrac{760\ \text{Torr}}{1\ \text{atm}} = 693.12\ \text{Torr}\)
02

b) Convert 0.685 bar to kilopascals

To convert 0.685 bar to kilopascals, we'll use the conversion factor 1 bar = 100 kPa: \(0.685\ \text{bar}\times \dfrac{100\ \text{kPa}}{1\ \text{bar}} = 68.5\ \text{kPa}\)
03

c) Convert 655 mm Hg to atmospheres

To convert 655 mm Hg to atmospheres, we'll use the conversion factor 1 atm = 760 Torr (or mmHg): \(655\ \text{mm}\ \text{Hg}\times \dfrac{1\ \text{atm}}{760\ \text{mm}\ \text{Hg}} = 0.8618\ \text{atm}\)
04

d) Convert 1.323 x 10^5 Pa to atmospheres

To convert \(1.323 \times 10^{5}\) Pa to atmospheres, we'll use the conversion factor 1 atm = 101325 Pa: \(1.323 \times 10^{5}\ \text{Pa}\times \dfrac{1\ \text{atm}}{101325\ \text{Pa}} = 1.306\ \text{atm}\)
05

e) Convert 2.50 atm to psi

To convert 2.50 atm to psi, we'll use the conversion factor 1 atm = 14.696 psi: \(2.50\ \text{atm}\times \dfrac{14.696\ \text{psi}}{1\ \text{atm}} = 36.74\ \text{psi}\)

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Most popular questions from this chapter

If 5.15 gof \(\mathrm{Ag}_{2} \mathrm{O}\) is sealed in a 75.0 - -mL tube filled with 760 torr of \(\mathrm{N}_{2}\) gas at \(32^{\circ} \mathrm{C},\) and the tube is heated to \(320^{\circ} \mathrm{C},\) the \(\mathrm{Ag}_{2} \mathrm{O}\) decomposes to form oxygen and silver. What is the total pressure inside the tube assuming the volume of the tube remains constant?

Suppose you are given two \(1-\) flasks and told that one contains a gas of molar mass 30 , the other a gas of molar mass 60 , both at the same temperature. The pressure in flask \(A\) is \(x\) atm, and the mass of gas in the flask is 1.2 \(\mathrm{g}\) . The pressure in flask \(\mathrm{B}\) is 0.5\(x\) atm, and the mass of gas in that flask is 1.2 \(\mathrm{g}\) . Which flask contains the gas of molar mass \(30,\) and which contains the gas of molar mass 60\(?\)

A sample of 5.00 \(\mathrm{mL}\) of diethylether \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OC}_{2} \mathrm{H}_{5},\right.\) density \(=0.7134 \mathrm{g} / \mathrm{mL}\) ) is introduced into a 6.00 -L vessel that already contains a mixture of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2},\) whose partial pressures are \(P_{\mathrm{N}_{2}}=0.751 \mathrm{atm}\) and \(P_{\mathrm{O}_{2}}=0.208\) atm. The temperature is held at \(35.0^{\circ} \mathrm{C},\) and the diethylether totally evaporates. (a) Calculate the partial pressure of the diethylether. (b) Calculate the total pressure in the container.

(a) What conditions are represented by the abbreviation STP? (b) What is the molar volume of an ideal gas at STP? (c) Room temperature is often assumed to be \(25^{\circ} \mathrm{C}\) . Calculate the molar volume of an ideal gas at \(25^{\circ} \mathrm{C}\) and 1 atm pressure. (d) If you measure pressure in bars instead of atmospheres, calculate the corresponding value of \(R\) in L-bar/mol-K.

On a single plot, qualitatively sketch the distribution of molecular speeds for (a) \(\operatorname{Kr}(g)\) at \(-50^{\circ} \mathrm{C},(\mathbf{b}) \mathrm{Kr}(g)\) at \(0^{\circ} \mathrm{C},\) (c) \(\operatorname{Ar}(g)\) at \(0^{\circ} \mathrm{C} .[\) Section 10.7\(]\)
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