An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. nitially, the temperature of the gas was 647.°C and had a pressure of 211. kPa. Determine the pressure of the gas when the temperature decreased to 154°C.

An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. nitially, the temperature of the gas was 647.°C and had a pressure of 211. kPa. Determine the pressure of the gas when the temperature decreased to 154°C.

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: Sulfur tetrafluoride gas is collected at 25.0 °C in an evacuated flask with a measured volume of…

Q: Calculate the molecular weight (molar mass) of a gas if 0.35 g of the gas at a temperature of 37.6…

Q: 2. A 0.136 g sample of an unknown metal (X) reacted with excess hydrochloric acid according to the…

A: According to ideal gas law PV = nRT where P = pressure in atm = P in mm Hg / 760 = 756 / 760 =…

Q: A certain gas has a volume of 29.5 L and a temperature of 44.5∞C. It then expands to a volume of…

Q: Chlorine pentafluoride gas is collected at −20.0°C in an evacuated flask with a measured volume of…

A: This can be calculated from ideal gas equation : PV = nRT

Q: A gas of unknown molecular mass was allowed to effuse through a small opening under…

A: According to Graham's law of effusion: The rate of effusion is also inversely proportional to the…

Q: Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose…

A: 8.80 L of Cl2 gas has a pressure of 890 torr at 23 °C .We have to calculate - A. Grams of Cl2 are…

Q: Consider a sample of air in a sealed container. Explain how the pressure of a gas would be affected…

A: 1) According to ideal gas law, PV = nRT where P = pressure V = volume n = moles R = gas constant T =…

Q: A) A sample of ideal gas at room temperature occupies a volume of 40.0 L at a pressure of 542 torr .…

A: Boyle’ law states that at a particular temperature and number of moles, the pressure of a gas is…

Q: Liquid nitrogen trichloride is heated in a 1.75-L closed reaction vessel until it decomposes…

A: Pressure of N2: 192 torr Pressure of Cl2: 577 torrExplanation:

Q: A gas mixture in a 4.900 L container at 310°C contains 1.25 g each of Ar, CO, and CH4. Find the…

A: The number of moles for a given chemical species refers to the ratio of mass of the species to that…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

A: Given: Note: 101.325 kPa = 1 atm Initially: Pressure of a gas (P1) = 252 kPa = 2.487 atm Temperature…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

A: Given :- Initial pressure (P1) = 295. KPa Initial temperature (T1) = 628.oC Final temperature (T2)…

Q: 891 mm Hg and a temperature of 65°C, occupies a volume of 17.9 liters. If the gas is heated at…

A: We have to find effect of temperature change on volume

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

A: Since the volume is kept constant we have to apply pressure law. The mathematical form of pressure…

Q: One of the factors that influences the behavior of a gas sample is pressure. Pressure can be…

A: Answer is explained below.

Q: Sulfur tetrafluoride gas is collected at 23.0 °C in an evacuated flask with a measured volume of…

A: Given that :The temperature of sulfur tetrafluoride gas = 23The volume of the gas = 15.0 LPressure =…

Q: A gas sample originally occupies 436mL at 24°C. When the volume is expanded to 612mL and the…

Q: A sample of ideal gas at room temperature occupies a volume of 15.0 L at a pressure of 752 torr. If…

A: Given, Note: 760 torr = 1 atm Initially: Pressure of a gas (P1) = 752 torr = 0.989 atm Volume of a…

Q: Suppose 10.05 mol of Ar gas are pumped into a 1.01 L container at 293.15 K. part 1:Calculate the…

A: Here we are required to find the pressure of Argon gas both ideally and non ideal scenario

Q: Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the…

A: Answer:Dalton's law of partial pressure states that partial pressure of any gas in the gaseous…

Q: A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas…

Q: An investigator is told that a closed vessel holds a pure rare gas. She measures the density of the…

A: The density of the gas, d = 0.8252 g/L Temperature of the gas, T = 298 K Pressure of the gas, P = 1…

Q: A 2.00 L sample of helium originally at 25 oC and a pressure of 745 torr is allowed to expand to a…

A: In all the gas laws (Boyle's, Charles' and Gay-Lussac's Law), pressure (P) and volume (V) remain in…

Q: A sample of helium at a pressure of 747 torr and in a volume of 2.09 L was heated from 22.5 to 74.6…

A: Given, P1=747 torrV1=2.09 LT1=22.5°C = 22.5+273 K = 295.5 KP2=?(final pressure)V2=2.81 LT2=74.6°C =…

Q: Hydrogen gas, oxygen gas, and water vapor are collected in eudiometer. The eudiometer contains…

Q: Some N₂ gas is mixed with some O2 gas, and the sketch below shows a representative sample of the…

A: given problem solved as Mole fraction = mole of one component ÷ mol of both componentsN 2 = 17÷ (…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

Q: A sample of gas has an initial volume of 3.96 L at a pressure of 708 mmHg. If the volume of the gas…

A: Consider the given information is as follows; Initial volume V1 = 3.96 LInitial pressure P1 = 708…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

Q: Sulfur tetrafluoride gas is collected at 28.0 °C in an evacuated flask with a measured volume of…

A: Given that : The temperature of sulfur tetrafluoride gas = 28°C The volume of the gas = 30.0 L…

Q: An empty glass flask has a mass of 56.52 g and a volume of 875.0 mL. When the flask is filled with…

A: Ideal gases are hypothetical gases which do have real existence. A gas can behave ideally at low…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

Q: Imagine that you measured the volume occupied by 2.8x10^-3 g of an unknown pollutant at standard…

A: Answer:Here:

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,25 L. Initially,…

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: convert between them

A: In order to convert a pressure unit to another one, we need to know the relationship between these…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

Q: Chlorine pentafluoride gas is collected at -17.0 °C in an evacuated flask with a measured volume of…

Q: An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially,…

Q: 1. Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atmatm and…

A: The objective of the first part of the question is to calculate the density of oxygen under two…

Q: . What is the mole fraction of each gas in a mixture having the partial pressures of 0.467 atm 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

100%

An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L.
Initially, the temperature of the gas was 647.°C and had a pressure of 211. kPa. Determine the
pressure of the gas when the temperature decreased to 154°C.

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: Given

VIEW

Step 2: Calculation of final pressure

VIEW

Solution

VIEW

Step by step

Solved in 3 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

5. You are given 1.56 g of a mixture of KClO3 and KC1. When the mixture is heated the oxygen gas liberated displaces 327 mL of water at a temperature of 19°C. The total pressure of the gas in the collection flask is 735 mmHg. What is the percentage of KClO3 in the mixture?
An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially, the temperature of the gas was 602.°C and had a pressure of 291. kPa. Determine the pressure of the gas when the temperature decreased to 157°C.
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
An engineer turns the temperature of a gas down, holding the volume constant at 1,250 L. Initially, the temperature of the gas was 684.°C and had a pressure of 208. kPa. Determine the pressure of the gas when the temperature decreased to 155°C.
Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr. key carbon hydrogen dlo nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr
A sample of gas at 1015.7 mmHg, occupying a volume of 14.66 L, and at a temperature of 21.31 °C is transferred to a container of 9.78 L with a pressure of 71.36 kPa. What is the new temperature in °C? Provide your answer with TWO decimals. Your Answer:
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.
Let 9.642 g He, 9.768 g F2, and 9.218 g Ar be placed in a 19.2-L container at 75°C. What are the molar concentrations and partial pressures of the gases? What is the total pressure in the container?
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?
Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 950. torr. key carbon hydrogen dh nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr
3. A certain mass of magnesium is reacted with 6M HCl. The hydrogen gas liberated is collected by displacing 200 mL of water. The pressure of the gas and the atmospheric pressure are equalized. The atmospheric pressure is 762 mmHg. The temperature of the experiment is 27°C. How many moles of hydrogen have been liberated, and what is the mass of the magnesium that reacted?