A 2.10 L sample of neon at 5.18 atm is added to a 12.0L cylinder that contains argon. If the pressure in the cylinder is 7.11 atm afterthe neon is added, what was the original pressure (in atm) of argon in the cylinder?Hint is given in the feedback.Answer:

Given, Volume of Neon gas is V1 = 2.10 L Pressure of Neon gas is P1 = 5.18 atm Volume of argon is V2…

Answered: A 2.10 L sample of neon at 5.18 atm is…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 152CP

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Similar questions

Given that 1.00 mol of neon and 1.00 mol of hydrogen chloride gas are in separate containers at the same temperature and pressure, calculate each of the following ratios. (a) volume Ne/volume HCI (b) density Ne/density HCI (c) average translational energy Ne/average translational energy HCI (d) number of Ne atoms/number of HCl molecules
Consider a 5.00-L tank containing 375 g of Ar at a temperature of 25 C. (a) Calculate the pressure in the tank using both the ideal gas law and the van der Waals equation. (b) Which correction term, a(n/V)2 or bn, has the greatest influence on the pressure of this system?
What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 C and 74-4 torr?
Describe what happens o the average kinetic energy of ideal gas molecules when the conditions are changed as follows: (a) The pressure of the gas is increased by reducing the volume at constant temperature. (b) The pressure of the gas is increased by increasing the temperature at constant volume. (c) The average velocity of the molecules is increased by a factor of 2.
Carbon monoxide, CO, and oxygen, O2, react according to 2CO(g)+O2(g)2CO2(g) Assuming that the reaction takes place and goes to completion, determine what substances remain and what their partial pressures are after the valve is opened in the apparatus represented in the accompanying figure. Also assume that the temperature is fixed at 300 K.
105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)

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A 2.10 L sample of neon at 5.18 atm is added to a 12.0L cylinder that contains argon. If the pressure in the cylinder is 7.11 atm after the neon is added, what was the original pressure (in atm) of argon in the cylinder? Hint is given in the feedback. Answer: