How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 27.0 L

Q: If 0.500 mol of helium gas occupies 5.00 L at 25 °C, what is the pressure in atmospheres?

A: Given details, n = 0.500 mol V = 5.00 L T = 25 °C = 298 K R = 0.08205 L.atm/mol.K To calculate the…

Q: A gas mixture has partial pressures of 52.55 mmHg H2, 159.74 mmHg N2, and 362.99 mmHg  O2. What is…

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Q: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 40.5 L?

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Q: What quantity in moles of oxygen gas at 140.0 °C and 43.3 atm would occupy a vessel of 2.85 L?

A: temparature (T): 140.0 °C = 413 k pressure (P) = 43.3 atm volume (V)=  2.85 L gas constant (R) =…

Q: If 1.04 g Ar are added to 4.83 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: We have to calculate the total gas pressure of mixture.

Q: What would be the mass (in kilograms) of a sample of gas with a molar mass of 34.08 g/mol held…

A: The pressure of 1 psi is equal to 0.068 atm. The temperature of 28.0oC in Kelvin is…

Q: Calculate the following quantities for an ideal gas: The absolute temperature of the gas at which…

A: Given, Number of moles of gas = 3.75 x 10-3 moles Temperature = ? Pressure of gas = 0.945 atm Volume…

Q: An isolated quantity of an ideal gas at 207.8 K has a volume of 31.21L at a pressure of 2.12 atm.…

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 26.5 L?

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

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 37.0 L?

A: Ideal gas equation is given by, PV=nRT

Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 14.5 L?

A: To solve this problem we will use Ideal gas equation which is given below as PV = nRT  Where,  P=…

Q: A 10.00 L tank at -2.9 °C is filled with 11.6 g of boron trifluoride gas and 3.29 g of dinitrogen…

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Q: A 8.00 L tank at 6.68 °C is filled with 11.4 g of dinitrogen difluoride gas and 6.23 g of chlorine…

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Q: A 6.96 gram sample of an unknown gas is found to occupy a volume of 2.10 L at a pressure of 912 mmHg…

A: Given that: mass of sample = 6.96 g volume of gas = 2.10 L pressure of gas = 912 mmHg temperature =…

Q: How many moles of CO2 are contained in 7.62 L at 38 °C and 711 torr?

A: Given -                         Volume of sample (V) = 7.62L…

Q: 2. Equal molar quantities of two gasses of molecular weight 4 and 40 are mixed. The pressure of the…

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Q: A 7.00 L tank at -5.1 °C is filled with 8.05 g of dinitrogen monoxide gas and 19.7 g of boron…

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 31.5 L?

A: Given,Temperature of chlorine, T = 120°CBut, K = °C + 273.15So, T = 393.15 KPressure, P = 33.3…

Q: A gaseous mixture consisting of 0.584 grams of H2(g) and 17.2 grams of N2(g) occupies 10.0 liters at…

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Q: Calculate the temperature in oC when 2.50 moles of argon occupy 25.0 L at 1.20 atm. Write the ideal…

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Q: Consider a gas mixture that contains only helium (He) and neon (Ne). If the partial pressure of He…

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Q: What quantity in moles of hydrogen gas at 150.0 °C and 23.3 atm would occupy a vessel of 8.50 L?

A: Given Pressure( P) = 23.3 atm Volume (V) = 8.50 L Temperature (T) = 150.0 oC Number of moles (n) = ?

Q: A gas sample containing 0.6838 moles is trapped in a chamber with a volume of 7.557 liters.  If the…

A: n = 0.6838 molV = 7.557 LT = 298.17 K

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 13.5 L?

A: The number of moles of chlorine can be calculated by using the ideal gas equation,

Q: What is the density (g/L) of H₂ gas at 0.640 bar and 50 °C?

A: Pressure of H2 gas = 0.640 barand temperature = 500CWe need to calculate the density (g/ml) of H2…

Q: partial pressure

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Q: sample of an ideal gas has a volume of 2.26 L at 2.90×10^2 K and 1.08 atm. Calculate the pressure…

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 24.0 L?

A: Calculate the temperature in Kelvin.

Q: What is the pressure of 1.51 g of nitrogen gas confined to a volume of 0.105 LL at 30 ∘C?

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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: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 34.5 L?

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Q: A 10.00 L tank at -7.6 °C is filled with 5.09 g of chlorine pentafluoride gas and 16.3 g of…

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Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 38.5 L?

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 14.0 L?

A: Temperature of Chlorine gas (T) = 120°C = 273+120 = 393K Pressure of Chlorine gas (P) = 33.3atm…

Q: Using Dalton's law of partial pressures, calculate the total pressure of a mixture of three gases,…

A: According to Dalton's law of partial pressures, the total pressure of a mixture of gases is equal to…

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

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Q: gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the…

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Q: What is the temperature of an 11.2 L sample of carbon monoxide, CO, at 7.44 atm if it occupies 13.3…

A: We can use combined gas law equation for this question.

Q: What quantity in moles of oxygen gas at 140.0 °C and 43.3 atm would occupy a vessel of 2.05 L?

A: Given -->  T = 140°C or 413.15 K  V = 2.05 L  P = 43.3 atm  R = 0.0821 L.atm/K.mol

Q: 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…

A: Answer:When number of moles of the gas is constant then ideal gas law for a gas is:Here:

Q: Calculate the following quantities for an ideal gas:

A: Given: Volume V=4.50 LPressure P=760.0 mmHg=1 atmtemperature T=25.0°C=298 Kuniversal gas constnat…

Q: A 16.0 L sample of argon gas has a pressure of 25.0 atm at a certain temperature. At the same…

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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.