Concept explainers
Interpretation: A gas is expanded from an initial volume of
Concept Introduction: The final pressure of the gas at the varying temperature and varying volumes can be calculated using combined
In combined gas law, the three laws of the gas are combined. Mathematically, it is given as
Two different sets of temperature and pressure of the gas is considered, the above equation becomes as follows:
Where
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Chapter 5 Solutions
Introduction to General, Organic and Biochemistry
- ➡ Listen ▶ Two flasks at the same temperature are joined by a glass tube with a stopcock. Flask A is 3.8 L flask containing N₂ (g) at 2.2 atm, while flask B is a 9.1 L flask containing CO (g) at 3.4 atm. What is the final pressure in the flask after the stopcock is opened? Answer to 1 decimal place.arrow_forwardReview I Constants I Periodic Table This figure (Figure 1) shows a container that is sealed at the top by a movable piston. Inside the container is an ideal gas at 1.00 atm, 20.0° C, and 1.00 L. This information will apply to the first three parts of this problem Part A What will the pressure inside the container become if the piston is moved to the 2.20 L mark while the temperature of the gas is kept constant? Express your answer with the appropriate units. View Available Hint(s) Value Units P = Submit Part B Figure 1 of 1 The gas sample has now returned to its original state of 1.00 atm, 20.0 °C, and 1.00 L. What will the pressure become if the temperature of the gas is raised to 200.0°C and the piston is not allowed to move? Express your answer with the appropriate units. View Available Hint(s) 2 L piston container ? μΑ F1L Value Units P = -ideal gas sample Submitarrow_forwardPart A A weather balloon is inflated to a volume of 25.5 L at a pressure of 738 mmHg and a temperature of 31.4 °C. The balloon rises in the atmosphere to an altitude where the pressure is 390. mmHg and the temperature is -15.6 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude. a) ? Vballoon = L Submit Request Answer What is the pressure if the volume of the container is maintained constant and the temperature is raised to 331 °C? Express the pressure in atmospheres to three significant figures. ΑΣφ. P = atm Submit Request Answer What is the density (in g/L) of hydrogen gas at 20 °C and a pressure of 1655 psi? Express your answer in grams per liter to three significant figures. • View Available Hint(s) Πνα ΑΣφ d = g/L Submitarrow_forward
- 4. A sample of a gas is in a 17.3 L container that is at a pressure of 0.33 atm and 34.3 °C. What is its new pressure if the Kelvin temperature was cut in half with the volume remaining constant? P₁ 163 Answerarrow_forwardA gas sample has an initial volume of 55.2 mL, an initialtemperature of 35.0 °C, and an initial pressure of 735 mmHg. The volume is decreased to 48.8 mL and the temperature is increased to 72.5 °C. What is the final pressure?(a) 933 mm Hg (b) 186 mm Hg(c) 1.72 × 103mm Hg (d) 401 mm Hgarrow_forwardExample 19 The volume in Liters of H (g) (measured at 22 "C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 C and 760 mmHg) in the reaction CO(g) + H2 (g) CH (g)+ HO(1) is: A) 63.5 L B) 74.1 L C) 77.2 L D) 70.0 Larrow_forward
- 0O REDMI NOTE 8 O BY DEEMA MAHMOUD A sample of a gas originally at 29°C and 2.25 atm pressure in a 3.0 L container is expanded until the volume is 5.2 L and the temperature is 11°C. The final pressure of the gas is torr. Select one: 445.6 927.7 842.4 1215.6arrow_forwardA sample of oxygen gas at a pressure of 1.16 atm and a temperature of 27.4 °C, occupies a volume of 13.3 liters. If the gas is allowed to expand at constant temperature to a volume of 21.2 liters, the pressure of the gas sample will be atm. Submit Answer Try Another Version 10 item attempts remainingarrow_forwardSolve Using Dalton’s Law of Calculate a Partial Pressure Problem 1. The total pressure exerted by a mixture of O2, N2, and He gases is 1.50 atm. What is the partial pressure, in the atmosphere, of the O2, given that the partial pressures of the N2 and He are 0.75 and 0.33 atm, respectively? Problem 2. A gas mixture contains O2, N2, and Ar at partial pressures of 125, 175, and 225 mm Hg, respectively. If CO2 gas is added to the mixture until the total pressure reaches 623 mm Hg, what is the partial pressure, in millimeters of mercury, of CO2?arrow_forward
- Attempt 2 A flexible container at an initial volume of 8.15 L8.15 L contains 7.51 mol7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 12.5 L.12.5 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.arrow_forwardCheck Your Understanding A mixture containing 13.5 g of oxygen and 60.4 g of N2 exerts a pressure of 2.13 atm at 25°C. What is the volume of the container, and what are the partial pressures of each gas? Answer + V = 29.6 L, Po, = 0.349 atm, PN, = 1.78 atmarrow_forwardName: CHEMISTRY PRACTICE PROBLEMS Avogadro's Law V _ V2 V,n, = V,n Assume that temperature and pressure are held constant for the following. 1. Determine the volume of 3.3 moles of hydrogen gas that is initially 5.7 moles at 7.53 L. 2. How many moles of CO2 will be left in a balloon that starts with 1.8 moles at 31 L when gas is allowed to escape to a volume of 25L? 3. A flexible container contains 6.02 x 1023 molecules of N, at a volume of 22.4L. What will be its new volume if the number of molecules is increased to 1.20 x 102? 4. A balloom starts with 5.8 x 10 molecules of N>O at 3.2-L What will-be the new-volume if the number of molecules is tripled? 5, How many molecules.of NH3 will.be left in a balloon that is deflated_to 0.5 L? The balloon starts with 7.8 x 1024 molecules at 46 L.arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning