A gas storage cylinder in an ordinary chemical laboratory measures 4.7 cm wide and 19. cm high.This is the label on it.Contents: N₂ gasPressure: 9.85 atmIf the cylinder is opened and the gas allowed to escape into a large empty plastic bag, what will be the final volume of nitrogen gas, including what's collectedin the plastic bag and what's left over in the cylinder? Write your answer in liters. Be sure your answer has the correct number of significant digits.

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Answered: A gas storage cylinder in an ordinary…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer. atm PNO atm Po, Incorrect atm PNO, Incorrect
What is the partial pressure of CO gas in a mixture of 0.400 moles of CO and 0.250 moles of H2S if the total pressure is 125 kPa? a. 81.3 kPa b. 50.0 kPa c. 31.3 kPa d. 76.9 kPa
Questions 7 through 11 refer to the information and diagram below. 2 NO2(g) > N204(g) NO2(8) reacts to form N20a(g) according to the equation above. A pure sample of NO2(g) is placed into a rigid, evacuated 0.500 L container. The initial pressure of the NO2(g) is 960 torr. The temperature is held constant until the NO2(g) reaches equilibrium with its product. The figure below shows how the pressure of the system changes while reaching equilibrium. Pressure (torr) 960 760 Time 8. The pressure vs. time curve can be used to evaluate (A) only the value of Q. (B) only the equilibrium constant from the horizontal part. (C) only the kinetics of the reaction from the decreasing part. (D) the kinetics of the reaction from the decreasing part and the equilibrium constant from the horizontal part.
Consider the reaction: 4 PH3 (g) → P4 (g) + 6 H2 (g) In the reaction above, 0.075 mole of H2 is produced in a 2.0-L container over some time period. What concentration of PH3 is consumed over the same time period?
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#15
A sample of Neon (Ne) gas is enclosed in a rigid 5.00 L container. At 300 K, the pressure on the walls of the container is 0.658 atm. 7a. How many moles of Ne are in the 7. container? 7b. How many Ne atoms are in the container? 8 7c. With the temperature held constant at 300 K, 0.267 mol of Ar (g) is injected into the rigid 5.00 L container with Ne (g) previously at 0.658 atm. What is the new total pressure and the partial pressures of Ne and Ar gases?
You are given the balanced equation: C3H8 + 5 02 3 CO2 + 4 H20 If 0.3618 moles of CaHg are allowed to react with 1.818 moles of O2, and this is the only reaction which occurs, what is the theoretical yield of water (in moles) that could be produced? O 1.456 moles O 1.447 moles O 2.180 moles . O 1.454 moles
In a fixed volume container at 25°C, NO2 gas partially combines to form N2O4 gas. The mass percentage of N2O4 in the resulting mixture is 76.3%, and the total pressure is 0.500 atm. What is the partial pressure of N2O4? A. 0.309 atm B. 0.619 atm C. 0.192 atm D. 0.119 atm E. 0.382 atm

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