Answered: A sample of nitrogen gas has a volume…

A sample of nitrogen gas has a volume of 478 cm³ and a pressure of 104.1 kPa. What volume would the gas occupy at 88.2 kPa if the temperature remains constant? Enter your answer in the box: 564 cm³

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...

See similar textbooks

Related questions

Q: Oxygen gas is collected at a pressure of 129 kPa in a container which has a volume of 11.5 L. What…

Q: A sample of gas contains 0.1600 mol of HBr(g) and 0.08000 mol of Cl₂ (g) and occupies a volume of…

A: As per Dalton's law, volume and number of moles are directly proportional to each other.

Q: A sample of gas is manipulated so that its temperature (in K) triples and its volume is reduced to…

A: An ideal gas will follow the ideal gas equation. The ideal gas equation is given by PV=nRT, where P,…

Q: Two samples of gas are separated in two rectangular 1.00 -L chambers by a thin metal wall. One…

A: Given: Volume = 1.00 L = 0.001 m3 Temperature =27oC = 27+273K = 300 K Pressure= 2.00 x 10-6 atm…

Q: A sample of argon gas at 55.19 °C has a pressure of 92.56 kPa and occupies 5.71 L. How many moles of…

A: In this question, we want to determine the number of moles of Argon gas You can see details…

Q: For many purposes we can treat nitrogen N2 as an ideal gas at temperatures above its boiling…

A: Answer:When number of moles of a gas is constant then equation of state for a gas sample is:Here:

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

A: Data

Q: A sample of argon gas occupies a volume of 0.0450 m³ at 101.3 kPa and 25.0°C. What volume would the…

Q: An engineer is preparing an experimental gas fuel mixture for a rocket launch. There are 5.00 g of…

A: Given

Q: A tank contains a mixture of 19.3 g of argon gas and 6.74 g of neon gas at 27 °C. The total pressure…

Q: A 9.60 L container holds a mixture of two gases, gas A and gas B, at 45 °C. The partial pressures of…

A: Here we are required to find the total pressure of the system .

Q: A tank contains a mixture of 14.6 g of argon gas and 9.69 g of neon gas at 27 °C. The total pressure…

A: We are having 9.69g Neon & 14.6g Argonnoof moles of Neon present = weight of Neon(g)Molar mass…

Q: A sample of 257.0 mL of wet nitrogen gas was collected over water at a total pressure of 759 torr…

Q: Which of the following is true for a gas under conditions of very low temperature? PV ÷ nRT = 1,…

A: To solve this problem we have to know about ideal gas equation.

Q: 7. Calculate the partial pressure of nitrogen and oxygen in a mixture of 35.8 grams of nitrogen gas…

Q: 1) At constant temperature, the volume of a gas is 275.0 mL at 850.0 mmHg. Calculate the volume of…

A: Boyle's law: According to Boyle’s law, the absolute pressure exerted by a given mass of an ideal…

Q: When heated, potassium chlorate decomposes to potassium chloride and oxygen gas according to the…

A: The objective of this question is to calculate the number of moles of potassium chlorate in the…

Q: A 10.0 gram mass of krypton occupies 15.0 L at a pressure of 156 kPa. Find the volume of the krypton…

A: According to ideal gas equation, PV = nRT The given problem will be solved keeping in mind that…

Q: A container holds a mixture of argon and nitrogen with a total pressure of 6.5 kPa. If the partial…

Q: partial pressure

Q: A sample of gas at 879.6 mmHg and occupying a volume of 14.39 L is transferred to a large container…

A: The given data: The initial pressure of the gas = 879.6 mmHg 1 mmHg = 0.133322 kPa 879.6 mmHg =…

Q: A sample of gas has a volume of 2.50 L at 916 kPa and 75.0 °C. What is the pressure (in atm) of the…

A: Given: P1 = initial pressure of gas = 916 kPa V1 = initial volume of gas = 2.50 L T1 = initial…

Q: At a certain temperature 65.2 mL of air, which is approximately 78% nitrogen, 21% oxygen and 1%…

A: Given : Initial volume of air = 65.2 mL Initial pressure of air = 105.3 KPa And final volume of air…

Q: A 190 mL sample of neon has its pressure changed from 75 kPa to 160 kPa. What is its new volume?

A: Given data, V1=190 mLP1=75 kPaP2=160kPa To calculate the new volume.

Q: A sample of gas at 867.5 mmHg, occupying a volume of 13.64 L, and at a temperature of 20.80 °C is…

A: P1 = 867.5mmHg V1 = 13.64L T1 = 20.80oC = 293.95K P2 = 255.09kPa = 1913.33207mmHg T2 = 74.66oC =…

Q: A 2.00 m3 container holds a sample of O2 gas. At 287 K the pressure of the container is 1.04 x 105…

A: Given, Volume of the container, V = 2.00 m3 = 2000…

Q: At 1.10 atm and 14.23 ∘C, a 2.15g sample of gas occupies a volume of 2.10×103 mL. Calculate the…

A: Given pressure = 1.10 atm volume = 2.10 × 103 ml Temperature = 14.23°C mass = 2.15 g

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling…

A: Initial Volume = V1 Final Volume = V2 Initial Temperature = T1 = −14.0°C = (−14.0 + 273.15) K =…

Q: A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr…

A: Introduction : Molarity is defined as the number of moles of solute dissolved in one litre of the…

Q: A sample of CO2 occupies a volume of 14.87 liters at 140.5 kPa. What pressure in kPa would the gas…

Q: A student collected 500. mL of nitrogen at a temperature of 20.°C. The next day the student found…

A: NOTE : Since you've asked multiple questions,we'll solve first question for you. If you want any…

Q: A sample of gas has a volume of 2.50 L at 781 kPa and 75.0 °C. What is the pressure (in atm) of the…

A: Given:P1 = 781 kPa = V1 = 2.50 LT1 = 75.0 oC = (75.0 + 273.15) K = 348.15 KV2 = 3.75 LT2 = 25.0 oC =…

Q: A sample of gas has a volume of 2.50 L at 536 kPa and 75.0 °C. What is the pressure (in atm) of the…

A: For the phase change of the ideal gas the temperature, pressure, and volume of the initial state and…

Q: A sample of 5.22 grams of xenon gas occupies a 500. mL container with a pressure of 565 kPa. What’s…

A: Given: Mass o Xenon = 5.22g Volume= 500 mL= 0.500L Pressure = 565 kPa = 5.59 atm To find: The…

Q: A sample of gas has a volume of 2.50 L at 761 kPa and 75.0 °C. What is the pressure (in atm) of the…

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

A sample of nitrogen gas has a volume of 478 cm³ and a pressure of 104.1 kPa.
What volume would the gas occupy at 88.2 kPa if the temperature remains
constant?
564 cm³
Enter your answer in the box: 564

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

A sample of gas has a volume of 2.50 L at 651 kPa and 75.0 °C. What is the pressure (in atm) of the gas if it expands to 3.75 L at 25.0 °C?
A sample of gas has a volume of 2.50 L at 556 kPa and 75.0 °C. What is the pressure (in atm) of the gas if it expands to 3.75 L at 25.0 °C?
ASK YOUR TEACHER A gas of unknown molar mass was allowed to effuse through a small opening under constant pressure conditions. It required 3650 s for 1.00 L of this gas to effuse. Under identical experimental conditions it required 471 s for 1.00 L of hydrogen (H2) gas to effuse. Calculate the molar mass of the unknown gas . (Remember that the faster the rate of effusion, the shorter the time required for effusion; that is, rate and time are inversely proportional.) a) The molar mass is 0.3 g/mol.b) The molar mass is 15.6 g/mol.c) The molar mass is 0.7 g/mol.d) The molar mass is 121.1 g/mol.e) The molar mass is 5.6 g/mol.
What is the mass (in g) of a 28.2 L sample of carbon dioxide gas at a temperature of 30.0 oC and a pressure of 113 kPa?
A 1.40 m3 container holds a sample of O2 gas. At 282 K the pressure of the container is 1.04 x 105 Pa. How many moles of O2 are in the container?
A 2.00 m3 container holds a sample of O2 gas. At 290 K the pressure of the container is 1.18 x 105 Pa. How many moles of O2 are in the container?
A gas mixture contains 1.0 mol neon, 2.0 mol argon, and 3.0 mol krypton in a 10.0 L flask at 0°C. Determine the partial pressure of neon.
4. In a laparoscopic surgery, carbon dioxide gas is used to inflate the abdomen to separate the internal organs and the abdominal wall. If the CO2 injected into the abdomen produces a pressure of 17 mmHg and a volume of 2.9 L at 26°C, how many moles of CO2 were used? How many grams? 5. What is the total pressure, in millimeters of mercury, of a gas mixture containing krypton gas at 0.45 atm and neon gas at 650 mmHg?
The ideal gas law, PV = nRT is independent of the kind of gas. In other words, the pressure exerted by a given number of ideal gas particles is the same whether the sample consists of all one type of particle or a mixture of different kinds of particles. Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Therefore, the pressure exerted by a mixture of gases can be expressed as follows: Part A Tota RT Ptotal = V What is the partial pressure of nitrogen in air at atmospheric pressure (101 kPa)? Assume ideal behaviour. A partial pressure is the pressure exerted by just one type of gas in a mixture. A partial pressure is calculated using only the number of moles of that particular gas, instead of the total number of moles: Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) RT P = V P = nRT P= nRT etc. The sum of the partial pressures is equal to the total…