A 4.00 L flask was filled with a mixture of equimolar amounts of nitrogen gas, and unknown gas at 27°C and 1.00 atm. The mixture had a mass of 10.0g. Calculate the molar mass of the unknown gas? Select one: a. 169g/mol O b. 218g/mol c. 95.2 d. 192g/mol e. 120g/mol

Q: I'm unsure of how to answer the question attached below the question is highlighted in red.

A: Number of moles of Kr and F can be calculated by the equation given below:

Q: A 1.9 mol sample of gas in a rigid flask at 21°C and 697 mm Hg is opened to the atmosphere and more…

A: Given, Initially, moles (ni) = 1.9 mol Pressure (Pi) = 697 mmHg Temperature (Ti) = 21°C = (21 +…

Q: Consider the following equation: CH&O7(s) +3 NaHCO3(s) + H20(1) --> Na3CgHgO7(s) + 3H2O(1) + 3CO2g)…

A: Here we first calculate the production of CO2 as a mole. Then use gas equation to determine the…

Q: A gas mixture is made by combining 5.3 g each of Ar, Ne, and an unknown diatomic gas. At STP, the…

A:

Q: A gas mixture is made by combining 8.7 g each of Ar, Ne, and an unknown diatomic gas. At STP, the…

A: Given : Conditions is STP i.e pressure = 1 atm and temperature = 273.15 K Mass of Ar = 8.7 g Mass of…

Q: A 4.00 L flask was filled with a mixture of equimolar amounts of nitrogen gas, and unknown 270C and…

A: The question is based on the concept of ideal gas equation. We have to calculate the molar mass of…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.00 atm of Gas A and 7.89 atm of Gas B. What is the…

A: Given Temperature T=25°C=298 KVolume V=10LPressure of gas A PA=5.00 atmPressure of gas BPB=7.89…

Q: A 0.4366 g sample of a compound of carbon, oxygen and hydrogen is burned completely and 453 mL of…

A: Given: mass of compound = 0.4366 g

Q: In a constant volume vessel, excessive H2 and 3.2 g O2 gas at 270 C create a pressure of 1.1…

A:

Q: 9. A gas exerts a pressure of 0.975 atm when at 20.0°C and in a 1.75 L vessel. A. How many moles of…

A: Use the ideal gas equation to find the moles of gas present,PV = nRT n = PVRT  Now n = moles of gas…

Q: and 27oC is cooled to -48oC at 608 torr.  a. What is the final volume?  b.  How many moles of gas…

A:

Q: References Use the References to access important values if needed for this question. A 1.97 gram…

A: Given, Mass of sample = 1.97g. Pressure = 692mmHg = 0.911atm. Volume = 1.15L. Temperature = 56oC =…

Q: At 1.35 atm and 5.91 °C, a 4.04 g sample of gas occupies a volume of 2060 mL. Calculate the molar…

A:

Q: The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen…

A: First write the reaction for magnesium metal with H2 and then check mol to mol ratio to calculate…

Q: A gas mixture is made by combining 7.2 g each of Ar, Ne, and an unknown diatomic gas. At STP, the…

A: The molar mass of Ar is 40 g/mol and that of Ne is 20 g/mol. Assume the molar mass of unknown to m…

Q: A steel tank starts with 1.241 moles of argon gas in it, with a pressure of 1.903 atm. 150.65…

A: * Initial condition of argon gas :-    Initial moles = 1.241 mol    Initial pressure = 1.903 atm…

Q: Determine the partial pressure and number of moles of each gas in a 18.50 L vessel at 33.9 °C…

A:

Q: A gas mixture is made by combining 8.1 g each of Ar, Ne, and an unknown diatomic gas. At STP, the…

A:

Q: #46 is the problem I need help with. How do you find the partial pressure of each with the…

A:

Q: At 25.0° C, a 10.00 L vessel is filled with 8.34 atm of Gas A and 7.89 atm of Gas B. What is the…

A: The gaseous state is the state of matter with least intermolecular force of attraction between…

Q: 0.9110 grams of an unknown gas was placed into an evacuated 0.500 L container. The temperature was…

A:

Q: .63 A mixture containing 0.765 mol He(g), 0.330 mol Ne(g), and 0.110 mol Arg) is confined in a…

A: Given data:

Q: A sample containing 0.2820 moles of a gas is trapped in a vessel at a temperature of 25.2 °C and a…

A:

Q: A 0.325 L flask filled with gas at 0.914 atm and 19 °C contains mol of gas. 0.0148 O 0.0124 O 40

A: The ideal gas equation is given by  PV = nRT  Given data Pressure inside the flask =0.914 atm V =…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.98 atm of Gas A and 7.89 atm of Gas B. What is the…

A:

Q: A 7.53 L cylinder contains 1.29 mol of gas A and 4.82 mol of gas B, at a temperature of 30.7 °C.…

A: Given that a 7.53 L contains 1.29 mol of gas A and 4.82 mol of gas B at a temperature of 30.7…

Q: Use the References to access important values if needed for this question. A 2.18 gram sample of an…

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

Q: A 1.31 gram sample of an unknown gas is placed in a 1.0 liter container at a temperature of 20°C and…

A:

Q: Titan's lower atmosphere is 94.2% nitrogen and 5.7% methane. The other 0.1% is composed of a…

A:

Q: In the reaction 2H₂ (g) +O₂ (g) = H₂ O₍₁₎ How many liters of oxygen gas at STP will be needed to…

A: The kinetic theory of gases stated that there are no forces of attraction between the particles of…

Q: A mixture contains 0.400 mol of gas A, 0.500 mol of gas B, and 0.120 mol of gas C. What is the total…

A:

Q: A chemist combines 11.8 L N2 gas, 33.9 L O2 gas, and 16.5 L Br2 gas in a reaction vessel at STP. The…

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

Q: A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0°C. (a) Calculate the density of the…

A: Given : Volume of vessel = 2.10 L  Mass of gas = 4.65 g Pressure of gas = 1.00 atm  And temperature…

Q: a) 1.488×10-4 mol of an unidentified gaseous substance effuses through a tiny hole in 81.2 s. Under…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.50 atm of Gas A and 7.89 atm of Gas B. What is the…

A: Partial pressure of gas A = 5.50 atm Partial pressure of gas B = 7.89 atm Total pressure of gas =…

Q: An unknown gas at 29.1 C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what…

A:

Q: At 25.0° C, a 10.00 L vessel is filled with 8.20 atm of Gas A and 7.89 atm of Gas B. What is the…

A: Given , volume of vessel = 10 L Temperature = 25C = 298 K

Q: A mixture of solid calcium oxide, CaO, and solid barium oxide, BaO, weighing 5.978 g is added to a…

A: Answer: In this question first of all we will calculate the moles CO2 consumed and then by the use…

Q: A 4.00 L flask was filled with a mixture of equimolar amounts of nitrogen gas, and unknown gas at…

A: Given: Mass of gaseous mixture = 10g Volume = 4L Temperature = 27°C = 300K Pressure = 1 atm

Q: An ideal gas is allowed to expand from 2.00 L to 7.00 L at constant temperature. By what factor does…

A:

Q: A steel tank starts with 1.241 moles of argon gas in it, with a pressure of 1.903 atm. 150.65…

A: The ideal gas equation is  PV = nRT  R = gas constant At constant volume and constant temperature ,…

Q: A 4.00 L sample of CO2 was collected over water at a total pressure of 1.56 atm and 20°C. The water…

A: Given data: Volume = 4.00 L Temperature = 20 oC = 293 K Total pressure = 1.56 atm

Q: 3. A 1.00-L sample of a gas at STP has a mass of 1.759 g. The molar mass of the gas is: [ Select)

A: Volume of gas at STP = 1.00 L Mass = 1.759 g

Q: 04. A sample of helium and neon gas occupy 1.30 L container at 45.0C. Calculate the partial pressure…

A:

Q: In a 10.0 L vessel at 100.0 °C, 10.0 grams of an unknown gas exert a pressure of 1.13 atm. What is…

A: Volume = 10L Temperature(T) = 100oc = 373K Mass of unknown gas= 10g  Molar mass of unknown gas =?…

Q: zadwany A 3.35 g sample of an unknown gas at 23 °C and 1.10 atm is stored in a 3.05 L flask. What is…

A:

Q: If a gaseous mixture is made by combining 3.56 g Ar3.56 g Ar and 2.13 g Kr2.13 g Kr in an evacuated…

A: The partial pressures of each gas has to be calculated The total pressure exerted by the gaseous…

Q: be a significant source of air pollution. The Kilauea volcano in Hawaii em 200–300t (1t= 10°kg) of…

A:

Q: 2. An unknown gas sample is collected in a 245 mL container at 25°C and 755 mmHg. a. How many moles…

A: Given :-  Volume of gas = 245 mL  Pressure  = 755 mm Hg  Temperature = 25°C  Mass of gas = 0.356 g…

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.