Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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12.1. A sample of gas has a pressure of 23.8 PSI and a volume of 250mL. If the volume is increased to 1.50 L, what will the new pressure be? Show calculations.
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- 2. Pressure Conversions a. Convert 0.650 atm to mm Hg. b. Convert 710.0 torr to atm.3. Temperature Conversions a. Convert 30.0 Celsius to Kelvin b. Convert 25 Celsius to Kelvin4. Name 4 factors that affect the properties of gasesSolve the following using the gas equations. Temperature must always be converted to kelvin before using in any equation. In addition to Kelvin for the Ideal Gas Law, pressure must be in atmospheres, volume in Liters, and n in moles. The gas constant with units is R=0.08206 (L atm)/(n K). Notice that the units of R dictate which units must be used for each parameter. Mind the significant figures in your calculations.5. Boyle’s Law - Temperature constant a. A sample of gas has a volume of 400.0 mL when measured at 25oC and 760.0 torr. What volume will it occupy at 25oC and 195.0 torr? b. What final pressure must be applied to a sample of gas having a volume of 200.0 mL at 20.0 oC and 750.0 torr pressure to permit the…arrow_forwardA sample of gas contains 0.1800 mol of and 0.09000 mol of and occupies a volume of 11.9 L. The following reaction takes place:2HCI(g) +Br_2(g) --->2HBr(g) +Cl_2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = ___ Larrow_forward7. The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two gases. a. What is the mole fraction of each gas in the mixture? b. If the mixture occupies a volume of 10.5 L at 65°C, calculate the total number of moles of gas in the mixture. C. Calculate the total mass of the mixture (hint, find the mass of each gas in the mixture). с. d. Calculate the relative rates of effusion for molecules of CH4 to that of a molecules of O2.arrow_forward
- 4. At constant volume, the temperature of 2.0 atm of gas was 325 K. The temperature is increased to 400 K. What is the new pressure of the gas?arrow_forward16. A gas with a pressure of 25.0 psi and a temperature of 18°C is heated to 24°C. What is the new pressure of this gas?arrow_forward1. At 27°C and 720 Torr, a certain gas sample has a volume of 765 mL. a. What would be its new volume if the temperature and pressure were changed to 57°C and 792 Torr? Hint: Use Combined Gas Law. b. How many moles are present in that gas sample? Hint: Use Universal Gas Law.arrow_forward
- A sample of hydrogen gas that occupies a volume of 31.9 L at a temperature of 0 °C and a pressure of 1 atm contains ___ moles of gas.arrow_forwardAccording to Charles’s law, the volume of a gas is directly related to its temperature in kelvins at constant pressure and the number of moles. In your initial post to the discussion, respond to the following prompts: What if there was an inverse relationship between the temperature and the volume? How do you think the world might be different? How would this change our day-to-day lives? Pick one of the following questions and try to answer it using one of the laws you learned in this module: How do spray cans work? Why do you need to fill up your tires with air on a cold day? Why do soda cans explode? When you inhale, your diaphragm increases in volume. How does this allow you to breathe? How does a syringe fill? How does filling a basketball with air increase its volume?arrow_forwardA sample of helium gas at a pressure of 1.08 atm and a temperature of 23.1 °C, occupies a volume of 15.1 liters. If the gas is allowed to expand at constant temperature to a volume of 21.1 liters, the pressure of the gas sample will be ______ atm.arrow_forward
- 3. A sample of 3.8 moles of a single gas is placed in a 5.500 L tube at 85.0 °C. The density of the gas is 2.76 g/L. What is the pressure of the gas in the tube? a. b. What is the molar mass of the gas in the tube?arrow_forwardA sample containing 4.70 gg of O2O2 gas has an initial volume of 11.0 LL . What is the final volume, in liters, when each of the following changes occurs in the quantity of the gas at constant pressure and temperature? A. A sample of 0.650 mole of O2O2 is added to the 4.70 gg of O2O2 in the container. B. A sample of 1.65 gg of O2O2 is removed from the 4.70 gg of O2O2 in the container. C.A sample of 4.80 gg of O2O2 is added to the 4.70 gg of O2O2 gas in the container.arrow_forwardA sample of nitrogen gas that occupies a volume of 45.5 L at a temperature of 0 °C and a pressure of 1 atm contains ________ moles of gas.arrow_forward
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