On venus the atmosphere consists primarily of carbon dioxide and nitrogen gas. If the partial pressure of carbon dioxide is 90.820 ATM and the partial pressure of nitrogen is 5.177atm what is the total pressure on Venus?

Q: Three gases (A, B, C) are mixed in a glass bulb. The total pressure inside the bulb is 0.40 atm.  If…

A: The objective of this question is to find the partial pressure of gas A in mmHg when the total…

Q: A sample of nitrogen gas has a pressure of 56.1 mm Hg in a 500. mL flask. What is the pressure of…

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Q: In a steel container of 5.00 L at 575 K, the partial pressures of H2(g) and O2(g) are, respectively,…

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Q: 5. A sample of air inside an Erlenmeyer flask occupies 135 mL and has a pressure of 946.3 mmHg and a…

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Q: 0.638 mol sample of xenon gas at a temperature of 25.0 °C is found to occupy a volume of 22.6…

A: number of moles = 0.638 mol Volume = 22.6 L Temperature = 25.0 °C = 298 K Gas constant , R =…

Q: A mixture of hydrogen and helium gases, in a 5.17 L flask at 36 °C, contains 0.390 grams of hydrogen…

A: Given, Volume of the flask (V) = 5.17 L Temperature (T) = 36°C = (36 + 273.15) K = 309.15 K Mass of…

Q: A container has an initial pressure of 2.82 atm and an initial volume of 46.2dL. The final volume is…

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Q: The pressure of a sample of argon gas was increased from 1.73 atm to 6.57 atm at constant…

A: Given data is as follows: The initial pressure of the gas P1= 1.73 atm The final pressure of the gas…

Q: A container of N2O3(g) has a pressure of 0.395 atm. When the absolute temperature of the N2⁢O3⁡(g)…

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Q: A helium-filled weather balloon has a volume of 729 L at 16.9°C and 755 mmHg. It is released and…

A: Initially,P1 = 755 mmHgV1 = 729 LT1 = 16.9°C = (16.9 + 273.15)K = 290.05 KLater,P2 = 454 mmHgV2 =…

Q: 0.743 mol sample of nitrogen gas at a temperature of 23.0 °C is found to occupy a volume of 20.7…

A: Since PV = nRT  where P = pressure in atm  V = volume in L = 20.7 L n = moles = 0.743 T =…

Q: A helium-filled weather balloon has a volume of 759 L at 20.9°C and 759 mmHg. It is released and…

A: Ideal gas equation  The equation that gives the relationship between temperature, pressure and…

Q: A helium-filled weather balloon has a volume of 774 L at 14.9°C and 753 mmHg. It is released and…

A: As you have posted two different questions and are not the sub-parts, so , here i have answered the…

Q: flask contains a mixture of N2 and H2 at a total pressure of 5.20 atm. If there are 1.00 mol of H2…

A: Given: Total pressure = 5.20 atm No.of mole of H2 = 1 mol No.of mole of N2 = 8 mol Calculate:…

Q: If the initial temperature of an ideal gas at 2.250 atm is 62.00 °C, what final temperature would…

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Q: A balloon filled with 2.00 L of helium initially at 1.15 atm of pressure rises into the atmosphere.…

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Q: 1. A 5.85 g sample containing only MgO and CuO is placed in a 5.00 L container. The container is…

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Q: A helium-filled weather balloon has a volume of 594 L at 18.9°C and 753 mmHg. It is released and…

A: Given,  A helium filled weather balloon has a volume of 594 L at 18.9 °C and 753 mmHg. After release…

Q: A mixture of xenon and argon gases, in a 9.94 L flask at 74 °C, contains 23.9 grams of xenon and…

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Q: A flask contains a mixture of oxygen, nitrogen, and hydrogen gases. If the partial pressure of…

A: • The values provided in the question are:-    i) Partial pressure of oxygen gas, PO2 = 546. 0 mm Hg…

Q: If a sample of Argon gas occupies 2.50 L at 100.0 °C and 5.00 atm, what volume will it occupy at 0.0…

A: The volume can be calculated as follows: P1V1T1  = P2V2T25.00atm×2.50L373K  = 1.00atm×V2273KV2=9.1 L

Q: A 2.20 L container at 53.6 °C contains 6.21g N2⁢O3⁡(g). The N2⁢O3 gas decomposes completely,…

A: Given :  Volume of vessel = 2.20 L  Temperature = 23.6 °C = 296.6 K  Mass of N2O3 = 6.21 g

Q: A mixture of methane and hydrogen gases is maintained in a 9.11 L flask at a pressure of 1.47 atm…

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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 =…