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Chapter 8: Problem 37

Freon-12 \(\left(\mathrm{CF}_{2} \mathrm{Cl}_{2}\right)\) is commonly used as the refrigerant in central home air conditioners. The system is initially charged to a pressure of 4.8 atm. Express this pressure in each of the following units ( 1 atm \(=14.7\) psi). a. \(\mathrm{mm} \mathrm{Hg}\) b. \(torr\) c. \(Pa\) d. \(psi\)

Short Answer

Expert verified
The given pressure of 4.8 atm is equivalent to: a. 3648 mmHg b. 3648 torr c. 486360 Pa d. 70.56 psi

Step by step solution

01

Conversion to millimeters of mercury (mmHg)

To convert the pressure from atm to mmHg, use the conversion factor 1 atm = 760 mmHg. The given pressure is 4.8 atm. \(4.8 \ \mathrm{atm} \times \frac{760 \ \mathrm{mmHg}}{1 \ \mathrm{atm}} = 3648 \ \mathrm{mmHg}\) Therefore, the pressure is 3648 mmHg.
02

Conversion to torr

To convert the pressure from atm to torr, use the conversion factor 1 atm = 760 torr. The given pressure is 4.8 atm. \(4.8 \ \mathrm{atm} \times \frac{760 \ \mathrm{torr}}{1 \ \mathrm{atm}} = 3648 \ \mathrm{torr}\) Therefore, the pressure is 3648 torr.
03

Conversion to Pascals (Pa)

To convert the pressure from atm to Pa, use the conversion factor 1 atm = 101325 Pa. The given pressure is 4.8 atm. \(4.8 \ \mathrm{atm} \times \frac{101325 \ \mathrm{Pa}}{1 \ \mathrm{atm}} = 486360 \ \mathrm{Pa}\) Therefore, the pressure is 486360 Pa.
04

Conversion to pounds per square inch (psi)

To convert the pressure from atm to psi, use the given conversion factor 1 atm = 14.7 psi. The given pressure is 4.8 atm. \(4.8 \ \mathrm{atm} \times \frac{14.7 \ \mathrm{psi}}{1 \ \mathrm{atm}} = 70.56 \ \mathrm{psi}\) Therefore, the pressure is 70.56 psi. So, the given pressure of 4.8 atm is equivalent to: a. 3648 mmHg b. 3648 torr c. 486360 Pa d. 70.56 psi

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Most popular questions from this chapter

Consider an equimolar mixture (equal number of moles) of two diatomic gases \(\left(A_{2} \text { and } B_{2}\right)\) in a container fitted with a piston. The gases react to form one product (which is also a gas) with the formula \(A_{x} B_{y}\). The density of the sample after the reaction is complete (and the temperature returns to its original state) is \(1.50\) times greater than the density of the reactant mixture. a. Specify the formula of the product, and explain if more than one answer is possible based on the given data. b. Can you determine the molecular formula of the product with the information given or only the empirical formula?

A container is filled with an ideal gas to a pressure of 11.0 atm at \(0^{\circ} \mathrm{C}\). a. What will be the pressure in the container if it is heated to \(45^{\circ} \mathrm{C} ?\) b. At what temperature would the pressure be 6.50 atm? c. At what temperature would the pressure be 25.0 atm?

Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. $$\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ Typically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 240\. mL of hydrogen gas is collected at \(30 .^{\circ} \mathrm{C}\) and has a total pressure of \(1.032\) atm by this process. What is the partial pressure of hydrogen gas in the sample? How many grams of zinc must have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at \(30^{\circ} \mathrm{C}\).)

A gas sample containing \(1.50\) moles at \(25^{\circ} \mathrm{C}\) exerts a pressure of \(400 .\) torr. Some gas is added to the same container and the temperature is increased to \(50 .^{\circ} \mathrm{C}\). If the pressure increases to \(800 .\) torr, how many moles of gas were added to the container? Assume a constant-volume container.

An organic compound containing only \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{N}\) yields the following data. i. Complete combustion of \(35.0 \mathrm{mg}\) of the compound produced \(33.5 \mathrm{mg} \mathrm{CO}_{2}\) and \(41.1 \mathrm{mg} \mathrm{H}_{2} \mathrm{O}\) ii. A 65.2 -mg sample of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129 ), giving \(35.6 \mathrm{mL}\) of dry \(\mathrm{N}_{2}\) at \(740 .\) torr and \(25^{\circ} \mathrm{C}\) iii. The effusion rate of the compound as a gas was measured and found to be \(24.6 \mathrm{mUmin.}\) The effusion rate of argon gas, under identical conditions, is \(26.4 \mathrm{mL} / \mathrm{min.}\) What is the molecular formula of the compound?
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