Concept explainers
Interpretation: The constant volume of the oxygen gas
Concept Introduction: The initial pressure of the gas at the varying temperatures can be calculated using Gay-Lussac’s law, which states the relationship between pressure and temperature of the gas
According to Gay-Lussac’s Law, for the gas held at constant volume, the pressure of a given amount of gas is directly proportional to the temperature of the gas. Mathematically, it is given as
We consider two different sets of temperature and pressure of the gas, the above equation becomes as follows:
Where
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Chapter 5 Solutions
Introduction to General, Organic and Biochemistry
- A sample of argon gas at a pressure of 762 mm Hg and a temperature of 22 °C, occupies a volume of 11.1 liters. If the gas is cooled at constant pressure to a temperature of -1 °C, the volume of the gas sample will be Submit Answer Try Another Version 10 item attempts remainingarrow_forwardTant values ilf needed for this question. A sample of neon gas occupies a volume of 9.83 L at 49.0°C and 0.700 atm. If it is desired to increase the volume of the gas sample to 11.4 L, while increasing its pressure to 0.914 atm, the temperature of the gas sample at the new volume and pressure must be PC. Submit Answer Try Another Version 2 item attempts remainingarrow_forwardWhat volume of oxygen gas is produced when 54.3 g of mercury(II) oxide reacts completely according to the following reaction at 25 °C and 1 atm? mercury(II) oxide (3) →mercury (1) + oxygen(g) 6.134 liters oxygen gas 6 more group attempts remaining Submit Answer Retry Entire Group The vapor pressure of liquid bromoethane, C,H¿Br, is 100. mm Hg at 263 K. A 0.376 g sample of liquid C,H&B is placed in a closed, evacuated 410. mL container at a temperature of 263 K. Assuming that the temperature remains constant, will all of the liquid evaporate?| What will the pressure in the container be when equilibrium is reached? mm Hg Submit Answer Retry Entire Group 8 more group attempts remainingarrow_forward
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- Check Your Understanding A mixture of SO2 (g) and SO3 (g) is to be prepared with a total pressure of 1.4 atm. If the mole fractions of the gases are 0.70 and 0.30, respectively, what are the partial pressures? If the mixture is to occupy 2.50 L at 27° C, what mass of each gas is needed? Answer + 6.4 g SO2, 3.4 g SO3 Pso2 = 0.98 atm, Pso, = 0.42 atmarrow_forwardProblem 2 Part a. The temperature of the gas is 22 degrees C. and it exerts a gas pressure of 740mmHg. What is the new pressure if the temperature increases to 35 degrees C? Part b. The temperature of the gas is 21 degrees C. And it exerts a gas pressure fo 545mmHg. What is the new pressure if the temperature increases to 25 degrees C? Part c. The temperature of the gas is 25 degrees C. and exerts a gas pressure of 695mmHg. What is the new pressure if the temperature increases to 37 degrees C?arrow_forwardExercise 6 Page 9 Illinois Central College CHEMISTRY 130 Name PRELAB: Exp.6 Gas Laws SHOW YOUR WORK 1.Ten (10.0) liters of hydrogen under 3.50 atm pressure is contained in a cylinder with a moveable piston. The piston is moved until the gas occupies only 3.00 liters. What is the new pressure of the cylinder? 2. A sample of gas at 25°C occupies 100.0 mL at atmospheric pressure, 740 mm Hg. If the pressure is increased to 800 mm Hg, what will be the new volume of the gas? 3. If 200 mL of oxygen at 100°C is heated to 200°C (the pressure remaining constant), what will be the new volume of the gas? 4. A 300 mL sample of hydrogen is measured at 27°C (room temperature). Assuming that the pressure does not change, at what temperature will the volume of this gas be 400 mL? 5. To what temperature must a gas sample at 20°C be heated in order to double its volume?arrow_forward
- M Review I Constants I Periodic Table Use the ideal gas law to complete the table: Complete the first column of the table. V 2.29 atm 1.24 L 209 K ΑΣφ les DA 519 torr 0.744 mol 299 K 0.423 atm 0.182 L 1.29x10-2 mol P = atm %3D 21.9 mL 5.81x10-3 mol 20.2 °C Submit Request Answer Part B Complete the second column of the table. ΑΣφ %3Darrow_forwardWhen extended, a bicycle pump has a volume of 0.952L at standard pressure (101.3 kPa). What is its pressure when the bicycle pump is compressed to a new volume of 0.225L and temperature remains constant? Answer: kPaarrow_forward9 Hint Resume Question 8 of 18 Question Two bulbs are connected by a stopcock. The 4.50 L bulb contains nitric oxide (NO) at a pressure of 0.273 bar, and the 1.50 L bulb contains oxygen (0,) at a pressure of 0.410 bar. NO After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (NO,). 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will decrease. There is not enough information to determine how the total pressure will change. The total pressure will remain constant. The total pressure will increase.arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning