Answered: When 7.00 moles of gas A and 3.00 moles…

When 7.00 moles of gas A and 3.00 moles of gas B are combined, the total pressure exerted by the gas mixture is 72.5 atm. What are the partial pressures exerted by each of the gases in this mixture?

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

Chapter5: Gases

Section: Chapter Questions

Problem 135AE

See similar textbooks

Related questions

Q: and 0.723 atm. If 0.140 mol of a third gas is added with no change in volume or temperature, what…

Q: If 45.5 g of O2 and 2.1 g of CO2 are placed in a 11.1 L container at 34 oC , what is the pressure…

Q: Consider this molecular-level representation of a mixture of gases. If the partial pressure of the…

A: partial pressure is the pressure exerted by individual gas molecules.

Q: Most mixtures of hydrogen gas with oxygen gas are explosive. However, a mixture that contains less…

A: First we are calculate presure of oxygen

Q: temperature

A: This question is related to ideal gas equation.

Q: If 42.0 g of O2 and 6.6 g of CO2 are placed in a 5.6 L container at 20 oC , what is the pressure…

A: Dalton's law: Dalton's law of partial pressures states that in a mixture of non-reacting gases, the…

Q: An experiment shows that a 110 mL gas sample has a mass of 0.170 g at a pressure of 744 mmHg and a…

Q: the pressure of a mixture of two gasses is 5.00 atm.If Gas A is 28%of mixture then what is the…

A: According to the Dalton's Law, Partial pressure of gas = mole fraction of gas X total pressure of…

Q: If a 2.51L sample of gas at 1.87atm is expanded to a final volume of 7.97L, what is the final…

A: Given Initial Volume ( V1 ) = 2.51 Liter Initial Pressure ( P1 ) = 1.87 atm Final Volume ( V2…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 4.70 moles of Gas B. What is the…

A: Given: Temperature of the system, T= 25.0°C = (25.0 + 273.15)K = 298.15 K Volume of the vessel, V…

Q: heliox deep-sea diving mixture contains 2.0 gg of oxygen to every 98.0 gg of helium. What is the…

Q: A sample of neon gas at 320 K and 0.762 atm occupies a volume of 1.89 L. If the compressed into a…

A: Given : initial pressure = 0.762 atm, initial volume = 1.89 L, initial temperature = 320 K. To find…

Q: A gas mixture with a total pressure of 2900 torrtorr is used by a scuba diver. If the mixture…

A: Numbers of moles is calculated by dividing the given mass with molecular mass of compound.

Q: A gas mixture contains 0.35 moles of Ne, 0.10 moles of He, and 0.39 moles of Ar. If the total…

Q: A sample of 12.4 liters of an ideal gas at 27.0 °C and 745.5 torr is compressed and heated so that…

A: The initial volume of the ideal gas is .The initial temperature of the ideal gas is .The initial…

Q: You have produced 170 g of NHin a 5.0L tank at 400.0 C. What is the total pressure of the gasses?

A: The relationship between temperature, pressure, volume and number of mole is given by ideal gas…

Q: Suppose a mixture containing 3.76 g H2 and 36.5 g NO has a total pressure of 2.02 atm. What are the…

Q: A mixture of gases containing 0.362 moles of oxygen, 1.23 moles of nitrogen, and 0.0234 moles of…

A: Given: moles of O2 = 0.362 mol moles of N2 = 1.23 mol moles of Ar = 0.0234 mol Total pressure = 2.60…

Q: If a gaseous mixture is made of 2.33 g of He and 2.82 g of Ne in an evacuated 1.25 L container at…

Q: At 35.0 °C, a 12.0 L vessel is filled with 6.25 moles of Gas A and 6.55 moles of Gas B. What is the…

A: o calculate the total pressure of the mixture of Gas A and Gas B in the given conditions, we need to…

Q: the pressure on a 2.66L volume of gas is 1.14atm and we decrease the volume of the container to…

A: We will use Boyle's law

Q: In a 10.00 L steel container, and at a temperature of 25.0°C, we have 76.0 g of O2(g) and 63.9 g of…

A: Given, The volume of the container, V = 10.00 LTemperature, T = 25.0oC = 298.15 KThe container…

Q: A sample of methane gas collected at STP occupies a volume of 49.7 L. How many moles of gas does the…

A: The moles of gas in a container depends on the volume, temperature, and pressure of the container.…

Q: A sample of hydrogen gas that occupies a volume of 37.7 L at a temperature of 0 °C and a pressure of…

A: The number of moles of a gas is calculated using the ideal gas equation. The ideal gas equation is…

Q: If a gaseous mixture is made of 2.93 g of He and 2.27 g of Ne and is in an evacuated 2.01 L…

A: The product of mole fraction with total pressure gives the partial pressure of a gas. Given volume…

Q: A mixture contains O2 at 700. torr pressure, F2 at 900. torr pressure, and Cl2 at 400. torr…

A: Given that, Pressure of O2=700 torr pressure of F2=900 torr pressure of Cl2=400torr then,

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 8.55 moles of Gas B. What is the…

A: According to Dalton`s law of partial pressure 'thr total pressure of a mixture of gases is equal to…

Q: At 45.0 °C, a 14.0 L vessel is filled with 7.25 moles of Gas A and 8.45 moles of Gas B. What is the…

A: From ideal gas law equation P•V = n•R•T P = pressure of gas V = volume R = gad constant T =…

Q: A mixture contains O2 at 429 torr pressure, F2 at 794 torr pressure, and Cl2 at 171 torr pressure.…

A: Total pressure is given by Dalton's law i.e. total pressure is equal to sum of partial pressure of…

Q: At 55.0 °C, a 16.0 L vessel is filled with 8.25 moles of Gas A and 1.00 moles of Gas B. What is the…

A: Information about the question

Q: A gas occupying a volume of 640.0 mL at a pressure of 0.834 atm is allowed to expand at constant…

A: The details solution for this is provided below in attach image.

Q: partial pressure

Q: Container A holds 712 mL712 mL of an ideal gas at 2.10 atm.2.10 atm. Container B holds 114 mL114 mL…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 4.65 moles of Gas B. What is the…

Q: At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100. liter container exert a…

A: Given : number of moles of H2 gas (n) = 4.0 mol volume (V) = 100. L pressure (P) = 1.00 atm To…

Q: At 55.0 °C, a 16.0 L vessel is filled with 8.25 moles of Gas A and 2.45 moles of Gas B. What is the…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 7.60 moles of Gas B. What is the…

Q: A mixture of 0.500 mol of Ne and 0.250 mol Ar have a total pressure of 3.20 atm. What is the partial…

Q: A mixture of 4.50 mol and H2 and 9.00 mol of O2 have a total pressure of 2.0 atm. What is the…

A: •partial pressure of any gas = mole fraction × total pressure.

Q: A mixture of gases contains: 2.70 g He, 8.13x1022 atoms of Ne, and 0.180 mol Ar. If the total…

Q: If the pressure exerted by a gas at 25.0oC in a volume of 0.0440 L is 3.81 atm, how many moles of…

A: The ideal gas law equation relates the pressure, volume, number of moles and the temperature…

Q: If 3.23 g Ar are added to 4.22 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

Q: At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100. liter container exert a…

A: The ideal gas equation for the relation between pressure (P), volume (V), temperature (T) is: PV=nRT…

Q: If 1.52 g Ar are added to 3.41 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

When 7.00 moles of gas A and 3.00 moles of gas B are combined, the total pressure
exerted by the gas mixture is 72.5 atm. What are the partial pressures exerted by each of
the gases in this mixture?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Partial Pressure

VIEW

Step 2: Mole Fraction

VIEW

Step 3: Partial Pressure

VIEW

Step 4: Answer

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A gas effuses through an opening one-fifth as fast as helium gas effuses through the same opening. (a) Is the gas heavier than helium? (b) What is the molar mass of the gas?
Shown below are three containers of an ideal gas (A, B, and C), each equipped with a movable piston (assume that atmospheric pressure is 1.0 atm). a How do the pressures in these containers compare? b Are all the gases at the same temperature? If not, compare the temperatures. c If you cooled each of the containers in an ice-water bath to 0.0C, describe how the volumes and pressures of the gases in these containers would compare.
The following figure shows three 1.00-L bulbs connected by valves. Each bulb contains argon gas with amounts proportional to the number of circles pictorially represented in the chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that the valves connecting the bulbs are closed and seal the gases in their respective chambers. Assume also that the volume between each bulb is negligible. (a) Which bulb has the highest pressure? (b) If the pressure in bulb A is 0.500 atm, what is the pressure in bulb C? (c) If the pressure in bulb A is 0.500 atm, what is the total pressure? (d) If the pressure in bulb A is 0.500 arm, and the valve between bulbs A and B is opened, redraw the figure shown above to accurately represent the gas atoms in all three bulbs. What is P A+P B+P C? Compare your answer in part (d) to that in part (c). (e) Follow the instructions of part (d) but now open only the valve between bulbs B and C.
Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation: HN3O(g)N2(g)+H2(g) If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.
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.
99 Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2dimerizes, or combines with itself, to produce a mixture of NO2 and N2O4. A particular mixture of NO2, and N2O4 has a density of 2.39 g/L at 50°C and 745 torr. What is the partial pressure of NO2 in this mixture?
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
Hydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.
47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?
Consider these four gas samples, all at the same temperature. The larger boxes have twice the volume of the smaller boxes. Rank the gas samples with respect to: (a) pressure, (b) density, (c) average kinetic energy, and (d) average molecular speed. (Green spheres are He; violet spheres are Ne.)