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Concept explainers
(a)
Interpretation:
The pressure exerted by
Concept introduction:
According to the
![Check Mark](/static/check-mark.png)
Answer to Problem 6.45E
The pressure exerted by
Explanation of Solution
The volume of the gas is
The temperature of the gas is
The number of moles of gas is
According to the ideal
Where,
•
•
•
•
•
Convert
Convert
The value of universal gas constant is
Substitute the value of number of moles, volume, temperature and gas constant in equation (1).
The pressure exerted by
(b)
Interpretation:
The volume of hydrogen gas in a steel cylinder is to be calculated.
Concept introduction:
According to the ideal gas law, the relation between pressure, temperature, volume and number of moles is,
![Check Mark](/static/check-mark.png)
Answer to Problem 6.45E
The volume of hydrogen gas in a steel cylinder is
Explanation of Solution
The pressure of the gas is
The temperature of the gas is
The number of moles of gas is
According to the ideal gas law, the relation between pressure, temperature, volume and number of moles is,
Where,
•
•
•
•
•
Convert
The value of universal gas constant is
Substitute the value of number of moles, pressure, temperature and gas constant in equation (2).
The volume of hydrogen gas in a steel cylinder is
(c)
Interpretation:
The temperature of a nitrogen gas is to be calculated.
Concept introduction:
According to the ideal gas law, the relation between pressure, temperature, volume and number of moles is,
![Check Mark](/static/check-mark.png)
Answer to Problem 6.45E
The temperature of a nitrogen gas is
Explanation of Solution
The pressure of the gas is
The volume of the gas is
The number of moles of gas is
According to the ideal gas law, the relation between pressure, temperature, volume and number of moles is,
Where,
•
•
•
•
•
Convert
The value of universal gas constant is
Substitute the value of number of moles, pressure, volume and gas constant in equation (3).
The temperature of a nitrogen gas is
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Chapter 6 Solutions
Chemistry for Today: General, Organic, and Biochemistry
- A typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.arrow_forwardA cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.arrow_forwardConsider the following sketch. Each square in bulb A represents a mole of atoms X. Each circle in bulb B represents a mole of atoms Y. The bulbs have the same volume, and the temperature is kept constant. When the valve is opened, atoms of X react with atoms of Y according to the following equation: 2X(g)+Y(g)X2Y(g)The gaseous product is represented as and each represents one mole of product. (a) IfP A=2.0 atm, what is P8 before the valve is opened and the reaction is allowed to occur? What is P A+P B? (b) Redraw the sketch to represent what happens after the valve is opened. (c) What is PA? What is PB? What is P A+P B? Compare your answer with the answer in part (a).arrow_forward
- Raoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.arrow_forwardA new boron hydride, BxHy, has been isolated. To find its molar mass, you measure the pressure of the gas in a known volume at a known temperature. The following experimental data are collected: Mass of gas = 12.5 mg Pressure of gas = 24.8 mm Hg Temperature = 25 C Volume of flask = 125 mL Which formula corresponds to the calculated molar mass? (a) B2H6 (b) B4H10 (c) B5H9 (d) B6H10 (e) Bl0H14arrow_forwardA study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O2 and CO2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 C [which means the partial pressure of water vapor in the lungs is P(H2O) = 47.1 mm Hg]. If you assume the lung gases consist of only O2, N2, CO2, and H2O, what is the partial pressure of N2?arrow_forward
- What does “STP’ stand for? What conditions correspond to STP? What is the volume occupied by one mole of an ideal gas at STParrow_forwardWhich of the following statements is(are) true? a. If the number of moles of a gas is doubled, the volume will double, assuming the pressure and temperature of the gas remain constant. b. If the temperature of a gas increases from 25C to 50C, the volume of the gas would double, assuming that the pressure and the number of moles of gas remain constant. c. The device that measures atmospheric pressure is called a barometer. d. If the volume of a gas decreases by one half, then the pressure would double, assuming that the number of moles and the temperature of the gas remain constant.arrow_forwardhe following demonstration takes place in a two-step process: rst, solid calcium carbide (CaC2j)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. Second the acetylene gas produced is then ignited with a match, causing the combustion reaction of acetylene with oxygen gas to produce gaseous carbon dioxide and gaseous water. Write the balanced equations for each reaction that is occurring, including all phases. If a 100.0gsample of calcium carbide (CaC2)is initially reacted with 50.0gof water, which reactant is limiting? Now imagine that the final gases produced are collected in a large bulkier and allowed to cool to room temperature. Using the information from part b ( l00.0gof Cec2reacting with 50.0gof H2O), how many liters of carbon dioxide gas were produced in the balloon at a pressure of 1.00atm and 25C?arrow_forward
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
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