At 46°C a sample of ammonia gas exerts a pressure of 980 torr. What is the pressure when the volume of the gas is reduced to one-fifth(1/5) of the original value at the same temperature?

Q: A sample of nitrogen gas has a pressure of 67.5 mmHg in a 500 mL flask. What pressure is this gas…

A: Solution: From Boyle's law we have PV = constant,  so we can write P1V1 =P2V2.

Q: A mixture of N2, O2, and CO2 has a total pressure of 749 torr. In this mixture the partial pressure…

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Q: A mixture of methane and helium gases, at a total pressure of 958 mm Hg, contains 1.90 grams of…

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Q: A balloon is filled with helium, and its volume is 2.2 L at 298 K and at atmospheric pressure. The…

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Q: A chemist has a 5.00 L gas-filled cylinder with a piston, at 25 o C. He pushes the piston part way…

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Q: At constant temperature the pressure on a 6.0 L sample of a gas is reduced from 1.00 atm to 1140…

A: Formula used: PV=nRT Given data: P1=1atm = 760torr P2=1140torr V1=6L

Q: A gaseous mixture of O2 and N2 contains 38.8 %% nitrogen by mass. What is the partial pressure

A: Assume Total mixture = 100 g  Mass of N2 = 38.8 g  Moles of N2 = 38.8 g/ 28 g/mol  = 1.38mol Mass…

Q: Which container shown below has the smallest partial pressure of argon? The white circles represent…

A: We have to tell which container had smallest portion of argon

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: What is the pressure of the sample of gas trapped in the open-end mercury manometer shown between if…

A: A manometer is used to measure the pressure of a gas. The manometer is of two types, both of which…

Q: Container A holds 757 mL of ideal gas at 2.50 atm . Container B holds 119 mL of ideal gas at 4.80…

A: Boyle's Law states that at constant temperature, the pressure of a fixed amount of gas varies…

Q: Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2…

A: The given chemical reaction is 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)  Total volume of the gas =…

Q: If a sample of gas occupying some volume has a pressure of 1.53 atm at 298 K, what is the pressure…

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Q: Three gases are present inside an 20.0L chamber. Argon is present at a partial pressure of 154 torr,…

A: Given that a 20.0L chamber contains,  Partial pressure of Argon gas pAr   = 154 torr Partial…

Q: A gas sample is prepared in which the components have the following partial pressures: nitrogen =…

A: Partial pressures (pN2) = 555 mm Hg Partial pressures (pO2) = 149 mm Hg Partial pressures (p water…

Q: A gas occupying a volume of 850 ml at a pressure of 1 atm is allowed to expand at constant…

A: Given information, Initial volume (V1) = 850 mL Initial pressure (P1) = 1 atm Final pressure (P2) =…

Q: 1. A sample of oxygen gas, which is saturated with water vapour, is kept in a 10- L vessel at 30°C…

A: Since you posted multiple questions, we answered the first two questions. We know that according to…

Q: A sample of methane, CH4, occupies a volume of 350.0 mL at 25°C and exerts a pressure of 1140.0…

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Q: At constant temperature, a sample of helium at 760. torr in a closed container was compressed from…

A: Given: The initial pressure of the helium gas (P1) = 760  The initial volume of the helium gas (V1)…

Q: A sample of CO2 was confined to a container at constant temperature. When the pressure applied to…

A: Given:: Initially, P1=6 atm , V1=5L

Q: At 56 degrees Celsius a sample of ammonia gas exerts a pressure of 7.5 atm. What is the pressure…

A: The ideal gas equation is given by, P1V1T1=constant where P is the pressure, V is the volume and T…

Q: At a constant temperature, a sample of helium at 760 torr in a closed container was compressed from…

A: Given, At a constant temperature, a sample of helium at 760 torr in aclosed container was compressed…

Q: What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if…

A: The gas pressure would be–  = 736 mm - 92 mm = 644 mm Hg

Q: A 300.-mL sample of hydrogen, H2, was collected over water at 21oC on a day when the barometric…

A: Pressure of Gas + Water = 748 torr Vapor pressure of water = 19 torr Pressure of H2 Gas = 748 -19 =…

Q: partial pressure

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Q: The total pressure exerted by a mixture of O2, N2, and He gases is 1.50 atm. What is the partial…

A: According to Dalton's Law of partial pressure, the total pressure exerted by a mixture of gases is…

Q: Synthetic diamonds can be manufactured at pressures of 6.00 x 10 4 atm. If we took 2.00 liters of…

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Q: A sample of nitrogen gas has a pressure of 175.0 mm Hg in a 500.0 mL flask.  What is the pressure of…

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

Q: 1.329 x 10–2 L of H2 (g) is collected over water at a total gas pressure of 744 torr and a…

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Q: A sample of helium gas at a pressure of 673 torr and a temperature of 24.8 celcius , occupies a…

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Q: A mixture of argon and xenon gases, at a total pressure of 719 mm Hg, contains 8.29 grams of argon…

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Q: A mixture of N2, O2, and CO2 has a total pressure of 749 torr. In this mixture the partial pressure…

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Q: The behavior of 485 mL of an ideal gas in response to pressure is studied in a vessel with a movable…

A: The equation which relates pressure, volume, temperature, number of moles and temperature with each…

Q: The temperature of a sample of gas in a steel container at 30.0 kPa is increased from -100.0°C to…

A: Volume of the steel container remain same.At constant volume recall the following relation…

Q: The temperature of a 500.mL sample of gas increases from 150. K to 350. K. What is the final volume…

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Q: A 7.94 g piece of solid CO 2 (dry ice) is allowed to sublime in a balloon. The final volume of the…

A: Given: mass of CO2 = 7.94 g Volume of balloon = 1.00 L Temperature = 301 K molar mass of CO2 = 44.01…

Q: A sample container of carbon monoxide occupies a volume of 422 mL at a pressure of 785 torr and a…

A: Write down the mathematical  expression for ideal gas law. PV=nRT Where P is the pressure of the…

Q: A mixture of N2, O2, and CO2 has a total pressure of 733 torr. In this mixture the partial pressure…

A: The partial pressure of CO2 can be calculated as follows

Q: If 150.00 mL of N2 gas was collected at 760 torrs, what is the new volume of the gas when the…

A: Boyles law: It stated that at constant temperature pressure of gas is inversely proportional to the…

Q: A sample of gas exerts a pressure of 635 torr in a 400 mL container at 25.0°C. What pressure would…

A: Given that : Initial volume (V1) = 400 mL Initial temperature (T1) = 25.0°C Initial Pressure (P1) =…

Q: pressure had increased to 15.0 atm,15.0 atm

A: The  final volume of balloon at pressure 15.0 atm. will be 0.0713 L

Q: A 250 mL container of CO2 exerting a pressure of 1.00 atm is connected through a valve to a 500 mL…

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Q: A gas occupies 0.850 liters at 1.00 atm and 27oC. What is the final temperature of the gas when the…

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

Q: What would be the volume of 3.90 moles of an ideal gas, at STP?  What is the pressure of this gas,…

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Q: A piece of solid carbon dioxide, with a mass of 7.8 g, is placed in a 4.0-L otherwise empty…

A: Given: Mass of carbon dioxide = 7.8g Volume of the container= 4L Temperature = 27°C= 27 + 273 = 300K

Q: A sample of nitrogen gas has a pressure of 70.5 mm Hg in a 610. mL flask. What is the pressure of…

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

Q: Dry air is 78.08% nitrogen, 20.95% oxygen, and 0.93% argon with 0.4% being other gases. If the…

A: Partial Pressure -  It is the pressure which would have been of a gas among many gases if it alone…

Q: pressure of the gas is increased, while at the same time it is heated to a higher temperature, the…

A:

Q: A sample of nitrogen gas occupies 9.20 L at 0.595 atm. If the pressure is increased to 2.15 atm at…

A: According to Boyle's law: The volume of a gas at constant temperature is inversely proportional to…

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.