Help me to answer this: 735The air taken from a newly discovered planet contains the following gases.concentration (%)20gascarbon dioxidehydrogenammonia401030охудenThe apparatus below was set up with a 100 cm3 sample of the air taken from the planet inthe graduated tube. The volume of the sample was measured at regular time intervals untilno further change in volume took place.-moist iron filingssample ofatmospherefrom planetgraduated tubewaterWhat is the volume of gas left in the tube?A20 cm3B30 cm370 cm380 cm3

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Answered: The air taken from a newly discovered…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 143CWP: A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon...

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93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
A mixture of 0.200 g of 1.00 g of and 0.820 g of Ar is stored in a closed container at STP. Find the volume of the container, assuming that the gases exhibit ideal behavior.
Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
The gas in the discharge cell of a laser contains (in mole percent) 11% CO2, 5.3% N2, and 84% He. (a) What is the molar mass of this mixture? (b) Calculate the density of this gas mixture at 32C and 758 mm Hg. (c) What is the ratio of the density of this gas to that of air (MM=29.0g/mol)at the same conditions?
A mixture of chromium and zinc weighing 0.362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, 225 mL dry of hydrogen gas was collected at 27C and 750. torr. Determine the mass percent of Zn in the metal sample. [Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium(III) chloride and hydrogen gas.]
If 1 cubic foot-28.3 L-of air at common room conditions of 230C and 0.985 bar is adjusted to STP, what does the volume become?
A 36.0—L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g 02, and 4,880 g N2. At 25 degrees C. what is the pressure in the cylinder in atmospheres?
Metallic molybdenum can be produced from the mineral molybdenite, MoS2. The mineral is first oxidized in air to molybdenum trioxide and sulfur dioxide. Molybdenum trioxide is then reduced to metallic molybdenum using hydrogen gas. The balanced equations are MoS2(s)+72O2(g)MoO3(s)+2SO2(g)MoO3(s)+3H2(g)Mo(s)+3H2O(l) Calculate the volumes of air and hydrogen gas at 17C and 1.00 atm that are necessary to produce 1.00 103 kg pure molybdenum from MoS2. Assume air contains 21% oxygen by volume, and assume 100% yield for each reaction.
A 275-mL sample of CO gas is collected over water at 31C and 755 mmHg. If the temperature of the gas collection apparatus rises to 39C, what is the new volume of the sample? Assume that the barometric pressure does not change.
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?
What is the density of laughing gas, dinitrogen monoxide, N2O, at a temperature of 325 K and a pressure of 113.0 kPa?
The barometric pressure measured outside an airplane at 9 km (30,000 ft) was 266 torr. Calculate the pressure in kPa.

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