Container A holds 787 mL of an ideal gas at 2.60 atm. Container B holds 164 mL of a different ideal gas at 4.40 atm. If the gases are allowed to mix together, what is the resulting pressure? P = TOOLS atm

Q: A gaseous mixture contains 0.170 mol of H2, 0.230 mol of N2, and 0.200 mol of Ne. The total pressure…

A: The partial pressure of a gas in a mixture is the product of total pressure and the mole fraction of…

Q: A 6.00 L tank at 17.4 °C is filled with 12.7 g of dinitrogen monoxide gas and 14.8 g of boron…

A: no. of moles = mass (g)molecular mass mole fraction = no of moles of one componenttotal moles given,…

Q: An ideal gas is contained in a cylinder with a volume of 5.1*102 mL at a temperature of 30.°C and a…

A: The combined gas law combines the three gas laws: Boyle's Law, Charles's Law, and Gay-Lussac's Law.…

Q: A sealed container holding 0.0255 L0.0255 L of an ideal gas at 0.987 atm0.987 atm and 69 ∘C69⁢ ∘C is…

A:

Q: The total pressure of gases A, B, and C in a closed container is 4.1 atmatm. If the mixture is 36%…

A: We know the gaseous mixture containing 36% of A, 42%of B, and 22% of C by volume,  Let consider the…

Q: Xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in a…

A: Let us consider the reaction between xenon and fluorine produces the compound XeaFb, where a and b…

Q: A 9.00 L tank at -8.5 °C is filled with 10.4 g of dinitrogen difluoride gas and 15.8 g of dinitrogen…

A: Given: Mass of dinitrogen difluoride i.e. N2F2 = 10.4 g. And mass of dinitrogen monoxide i.e. N2O =…

Q: Dinitrogen difluoride gas is collected at 13.0 °C in an evacuated flask with a measured volume of…

A: Given  Temperature ( T ) = 13 ℃                              = ( 13 + 273 ) K…

Q: A 7.00 L tank at 8.83 °C is filled with 17.0 g of sulfur hexafluoride gas and 10.5 g of boron…

A: First we will calculate the number of moles of  each gas . Than calculate the partial pressure of…

Q: A 7.00 L tank at -6.3 °C is filled with 18.4 g of dinitrogen difluoride gas and 4.58 g of dinitrogen…

A:

Q: A 10.0 L tank at 23.7 °C is filled with 5.14 g of boron trifluoride gas and 13.4 g of dinitrogen…

A:

Q: An unknown gas at 25.1 ∘C25.1 ∘C and 1.10 atm1.10 atm has a molar mass of 44.10 g/mol.44.10 g/mol.…

A:

Q: An ideal gas originally at 0.85 atm and 65°C was allowed to expand. until its final volume,…

A: Ideal gas law ,   Ideal gas law state the relation between the pressure, temperature, volume and…

Q: e identity of the gas?

A:

Q: A 10.0 L tank at 2.58 °C is filled with 14.4 g of sulfur hexafluoride gas and 2.83 g of dinitrogen…

A: Given, volume of the tank =10.0 Ltemperature T =2.58 °C =(2.58+273.15) K =275.73 Kamount of sulfur…

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

A: Answer is explained below.

Q: A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 g of dinitrogen…

A:

Q: A 10.0 L tank at 1.79 °C is filled with 15.7 g of sulfur tetrafluoride gas and 15.1 g of dinitrogen…

A: Moles of SF4 =  15.7 g /108gmol-1                          = 0.145 mol Moles of N2F2 = 15.1 g /66…

Q: A rigid container with a fixed volume is filled with 1.0 mole of nitrogen gas (N2) at 0.5 atm…

A: The given information is as follows: The moles nitrogen gas n1 = 1.0 mole The initial pressure of…

Q: Container A holds 737 mL of an ideal gas at 2.90 atm. Container B holds 169 mL of a different ideal…

A: The total pressure is determined by using the following formula

Q: Container A holds 742 mL of an ideal gas at 2.30 atm. Container B holds 169 mL of a different ideal…

A: Given, Gas in Container A Volume of gas A = 742 mL Pressure of gas A = 2.30 atm Gas in Container B…

Q: 5. A mixture of gases contains 10.25g of F2, 2.83g of H₂, and 5.95g of CO₂. If the total pressure of…

A:

Q: The total pressure of a gas mixture in a particular container is 43.2 atm. The flask contains 2.87…

A: total pressure = PT = 43.2 atm  mole of argon = 2.87 mole of chlorine = 7.40 mole of xenon = 15.2…

Q: If a gas initially had a volume of 16.9 L when its pressure was 1.53 atm, find the new volume of the…

A: At constant temperature pressure is inversely proportional to volume.

Q: Container A holds 737 mL737 mL of an ideal gas at 2.60 atm.2.60 atm. Container B holds 174 mL174 mL…

A: The total pressure is determined by using the following formula

Q: A 9.00 L tank at 4.56 °C is filled with 8.55 g of chlorine pentafluoride gas and 9.34 g of…

A: Number of moles of any Substance can be calculated by - Moles = mass/Molar mass Here, Mass of…

Q: gas mixture is made of 3 various gases. there are 0.254 moles of gas 1, 1.15 moles of gas 2, and…

A:

Q: Container A holds 772 mL of an ideal gas at 2.80 atm.Container B holds 139 mL of a different ideal…

A: Given, ideal gases as follows,volume of gas in container A =772 mL =0.772 Lat pressure =2.80…

Q: A 7.00 L tank at 12.3 °C is filled with 12.8 g of sulfur hexafluoride gas and 15.5 g of sulfur…

A: Given: Volume of tank = 7 L Temperature = 12.3°C=12.3+273.15 K=285.45 K Mass of sulfur hexafluoride…

Q: Container A holds 782 mL of an ideal gas at 2.70 atm.Container B holds 179 mL of a different ideal…

A: Resulting Pressure after Mixing can be calculated by the expression used in step-2   Pnet• =…

Q: A sealed container holding 0.0255 L of an ideal gas at 0.981 atm and 67 °C is placed into a…

A: According to Gay-Lussac's law for an ideal gas, the pressure of a gas is directly proportional to…

Q: Container A holds 762 mL of an ideal gas at 2.30 atm. Container B holds 159 mL of a different ideal…

A: Since the gases are allowed to mix together, So the resulting pressure can be calculated as…

Q: A gas originally at 25oC and 1.50 atm pressure in a 2.3 liter container is allowed to expand until…

A:

Q: 10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 g of sulfur…

A: Given: Volume of tank = 10.0 L Mass of dinitrogen difluoride = 15.4 g Mass of sulfur tetrafluoride…

Q: A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen…

A:

Q: If the initial temperature of an ideal gas at 2.250 atm2.250 atm is 62.00 ∘C,62.00 ∘C, what final…

A: Initial temperature (T1) = 62.00 ◦C Initial pressure (P1) = 2.250 atm Final pressure (P2) = 1.700…

Q: At 1.01 atm and 5.66 ∘C a 2.51 g sample of gas occupies a volume of 2430 mL. Calculate the molar…

A: Given,  pressure = 1.01 atm Volume = 2430 ml = 2.43 L  Mass of gas = 2.51 g Temperature = 56.6°C =…

Q: An ideal gas in a sealed container has an initial volume of 2.40 L. At constant pressure, it is…

A: Given data: V1 = 2.4 L V2 = 1.75 L T2=16oC   =(16+273) K=289 K  To find: T1=?

Q: A gas sample occupying a volume of 87.5 mL at a pressure of 0.887 atm is allowed to expand at…

A: According to Boyle's law, the relation between the volume of the gas and the pressure of the gas are…

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

A:

Q: Container A holds 797 mL of an ideal gas at 2.50 atm. Container B holds 174 mL of a different ideal…

A: For gas in container A, Pressure, P1 = 2.50 atm Volume, V1 = 797 mL   For gas in container B,…

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: A 9.00 L tank at 22.4 °C is filled with 11.2 g of boron trifluoride gas and 13.3 g of sulfur…

A: Volume of tank = 9L Temperature = 22.4°C or 295.55K Mass of boron trifluoride = 11.2g  Mass of…

Q: An ideal gas originally at 0.85 atm and 62°C was allowed to expand until its final volume, pressure,…

A: P1V1/T1 = P2V2/T2 V1 = P2V2T1/P1T2

Q: The mole fraction of hydrogen gas in a mixture of gases is 0.17. The total pressure of the gas…

A: Partial pressure of a gas can be calculated from the total pressure of the gas mixture if we somehow…

Q: A gas mixture contains 0.1044 mol of N2 and 0.0740 mol of HI. What is the partial pressure of N2, if…

A: It is an example of Dalton Law

Q: A 6.00 L tank at -2.6 *C is filled with 18.9 g of sulfur tetrafluoride gas and 9.34 g of dinitrogen…

A:

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.