If the number of moles of a gas increases at constant temperature and volume, how does the pressure of the gas change?а.Increaseb. Decreasec. Remain unchangedd. There is insufficient information to tell

Answer - The correct option is (a) = Increase According to the question - Given - The pressure…

If the number of moles of a gas increases at constant temperature and volume, how does the pressure of the gas change? a. Increase b. Decrease c. Remain unchanged d. There is insufficient information to tell

If the number of moles of a gas increases at constant temperature and volume, how does the pressure of the gas change? a. Increase b. Decrease c. Remain unchanged d. There is insufficient information to tell

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter13: Gases

Section: Chapter Questions

Problem 78A

See similar textbooks

Related questions

Q: A 1.00 mol of helium, He gas fills up an empty balloon to a volume of 1.50 L. Calculate the volume…

A: At the constant pressure and temperature, the volume of the ideal gas is directly proportional to…

Q: A. For a sample of gas at constant temperature, its pressure multiplied by its volume is constant.…

A: To solve this question, we need to check the gaseous law like boyle's law, charle's law,…

Q: Is the volume of a gas directly or inversely proportional to the numberof moles of a gas at constant…

A: This problem can be solved by using the ideal gas equation: PV = nRT where P is the pressure of the…

Q: Charles' Law states that, for a gas at constant pressure a. the volume increases as the temperature…

A: Charles law : At constant pressure, volume occupied by gas is directly proportional to its absolute…

Q: List the standard conditions for gas measurements.

A: Standard conditions for gas measurements are used when calculations are performed assuming the gases…

Q: The stopcock connecting a 3.27 L bulb containing xenon gas at a pressure of 8.26 atm, and a 3.86 L…

A: Given information, Volume of xenon gas is 3.27 L Pressure of xenon gas is 8.26 atm Volume of methane…

Q: Jacques Charles found that increasing the temperature of a gas sample at constant pressure would…

Q: Boyle's Law deals with the relationship between a. pressure and temperature b. volume and…

A: Boyle's law – Boyle’s law is a gas law which states that the pressure exerted by a gas (of a given…

Q: What happens to the average speed of gas molecules as the temperature increases? Why?

A: According to Kinetic Theory of Gases, The average speed is mathematically represented…

Q: nt pressure, the volume of a gas is directly proportional to the urc of a gas.

A: True statement is 2,4,5

Q: Attached is Charles’ Law Displayed Graphically. What is the temperature when the volume is equal to…

A: We have to tell the temperature when the volume is equal to zero and what this indicates. According…

Q: One way to state Boyle’s law is “All other things being equal, the pressure of a gas is inversely…

A: The ideal gas equation is as follows, Where, P is…

Q: How can we calculate the new volume if the pressure and temperature of this fixed number of moles…

A: How to calculate the new volume if the pressure and temperature of this fixed number of moles of…

Q: 23. Which equation is incorrect? Assume that T1 and T2 are in Kelvin units. A. V2/V1 = P1/P2, for a…

A: Various gas laws have been given that provides a relationship among pressure, volume and temperature…

Q: Consider a sample of gas that contains 625 moles of smokestack gas. How many molecules of SO, are…

Q: How do gas particles respond to an increase in temperature?A,There is a decrease in kinetic energy…

Q: If the TEMPERATURE of a gas is HALVED and the VOLUME of the gas is DOUBLED, how will the PRESSURE be…

Q: At standard temperature and pressure, a 1.00 mol sample of Argon gas is vented into a 22.4 L rigid…

A: At standard temperature and pressure N2 act near about as an ideal gas. Argon is an ideal gas Given…

Q: Increasing the volume of a given amount of gas at constant temperature causes the pressure to…

A: Increasing the volume of a gas decreased the pressure at a constant temperature because : a) the…

Q: the temperature of a gas decreases, it can be concluded that the volume of the gas will- stay the…

Q: An 1.50 mol sample of neon gas at a temperature of 20.0°C is found to occupy a volume of 21.9…

A: Given Number of mole = 1.50 mole Temperature = 20℃ = (20 + 273)…

Q: An 1.28 mol sample of carbon dioxide gas at a temperature of 6.0°C is found to occupy a volume of…

Q: One way to increase pressure of a gas is to (a) decrease temperature. (b) increase volume. (c)…

A: Since PV = nRT as per ideal gas law where P= pressure V = volume n = moles R = constant T =…

Q: A) The volume of a gas is directly proportional to the temperature of the gas. B) The pressure of a…

A: Charles law is defined for volume and temperature

Q: maintaing a constant pressure the volume of a gas is increased from 18L to 32L by heating it. if the…

A: new temperature?

Q: "The pressure of an ideal gas is inversely proportional to its volume at constant temperature and…

A: Gases that obey Boyle's law and Charle's law are known as ideal gases. According to Boyle's law at…

Q: Charles law states that for a fixed sample of gas at a constant temperature, pressure is inversely…

A: Charles Law states that the volume of an ideal gas at constant pressure is directly proportional to…

Q: Gas pressure for a mixture of nitrogen and helium is determined by a. the total number of particles…

Q: If temperture and pressure remain constant, how does the volume of a gas sample vary with the number…

A: This can be solved using ideal gas equation, According to this equation P V = n R T T is…

Q: The stopcock connecting a 2.0S L bulb containing neon gas at a pressure of 6.99 atm, and a 3.29 L…

Q: The average molecular speed in a sample of N2 gas at a certain temperature is 479 m/s. The average…

Q: References Use the References to access important values if needed for this question. A sample of…

A: Given, initial Temperature = 247°C Volume = 644 mL Final Volume = 546 mL Final temperature = ?

Q: If one atmosphere of pressure is equal to 760 torr, a pressure of 675 torr is equal to what value in…

A: 1 atm = 760 torr

Q: According to Boyle's law as the pressure of a gas increases its volume decreases increases…

Q: According to Charles's law, a gas will have a decreased if the volume is reduced. a) average kinetic…

Q: 15) A sample of gas at STP occupies 1.12 L at STP and has a mass of 1.007g. Determine the molar mass…

Q: .For each pair of variables, state whether they vary directly or inversely for a gas. a. pressure…

A: a. Pressure and volume - they vary indirectly As per Boyle's law, At fixed mass of gas and…

Q: When a volume of gas is heated at a specific temperature, the volume of the gas is expected to…

A: The correct option is (a) The volume will increase. It is because when the temperature increases,…

Q: If the absolute temperature of a gas is doubled and the pressure of the gas is halved, how will the…

A: According to ideal gas law, PV = nRT where P = pressure V = volume n = moles R = gas constant =…

Q: A gas has a volume of 4.23 L at 0°C. What final temperature, in degrees Celsius, is needed to change…

Q: Given the formula for The Gas Law: PV = nRT. Katie tried to solve for the V variable in order to…

A: The gas laws are the law that shows the behavior of any gas on the basis of the following…

Q: a For the following set of pressure/volume data, calculate the missing quantity. Assume that the…

A: By using Boyles law, Pressure is inversely proportional to its volume at constant Temperature. ie;…

Q: 1. 1/4 mole of 02 gas and 0.15 mol of hydrogen gas are mixed in a liter container at a temperature…

Q: 15. A rigid steel tank containing argon gas has additional argon gas pumped into it at a constant…

A: We would use ideal gas laws and given conditions to determine true statement.

Q: 10) Starting with an ideal gas particle bouncing around in a cube, derive the relationship between…

Q: An 1.09 mol sample of oxygen gas at a temperature of 25.0°C is found to occupy a volume of 26.3…

A: Given, number of moles of O2 = 1.09 moles Volume = 26.3 L Temperature = 25°C = 273+25 = 298 K

Q: If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is…

A: The change in volume of the air in the balloon if the pressure is constant has to be given,

Q: Use the kinetic molecular theory of gases to predict what would happen to a closed sample of a gas…

A: Since the average kinetic energy of the gas depends only on the temperature.

Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

Question

If the number of moles of a gas increases at constant temperature and volume, how does the pressure of the gas change?
а.
Increase
b. Decrease
c. Remain unchanged
d. There is insufficient information to tell

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 images

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

Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
Referring to exercises 1.6 and 1.7, does it matter if the pressure difference is caused by an ideal gas or a non-ideal gas? Explain your answer.
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
A tank is filled with gas to a pressure of 875 mm Hg at 25C. The gas is transferred without loss to a tank twice the size of the original tank. If the pressure is to remain constant, at what temperature (in C) should the tank be kept?
2.50Lcontainer at 1.00atm and 48Cis filled with 5.41gof a monatomic gas. Determine the identity of the gas. Assuming the 2.50Lcontainer is a large elastic balloon, predict what will happen when 10.0gof oxygen gas is added to the balloon (which already contains 5.41gof the monatomic gas). ovide values for each of the following variables. In addition, explain what is happening for each variable, incorporating the kinetic molecular theory into your explanation. m>Temperature of gas mixture = ?K m>Total moles of gas mixture = ?mol m>Total pressure of gas mixture = ?atm m>Volume of balloon = ?L Now assuming the 2.50Lcontainer is rigid (like a steel container), predict what will happen when 10.0gof oxygen gas is added to the container (which again already contains 5.41gof the monatomic gas). ovide values for each of the following variables. In addition, explain what is happening for each variable, incorporating the kinetic molecular theory into your explanation. m>Temperature of gas mixture = ?K m>Total moles of gas mixture = ?mol m>Total pressure of gas mixture = ?atm m>Volume of rigid container = ? L
A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?