The density of an unknown gas is found to be 2.89 g/L at 124°C and 141 atm. Find the molar mass of the gas.

Q: A sample of carbon dioxide is contained in a 500.0500.0 mL flask at 0.9760.976 atm and 15.615.6 ∘∘C.…

A: Given, Volume of the flask = 500.0 ml = 0.5 L pressure = 0.976 atm Temperature = 15.6 C° = (15.6 +…

Q: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 5.00 moles of Gas B. What is the…

A: Given-> Temperature (T) = 25.0°C = 25.0 + 273 = 298 K Volume of vessel (V) = 10.00 L Moles of A =…

Q: (a) Calculate the density of NO2 gas at 0.970 atm and 35 °C. (b) Calculate the molar mass of a gas…

A: (a). Using the ideal gas equation, the concentration of NO2 is determined as,

Q: A sample of gas occupies a volume of 101 mL at 220.0 torr and 30.5˚C. Calculate the volume at 500.0…

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

Q: An unknown gas has a volume of 200.L at atm and -140 celcius. what is its volume at STP?

A:

Q: . In a hospital an oxygen cylinder contains 423 L of pure oxygen at a pressure of 136 atm. What is…

A: In this question, we will determine the volume of oxygen gas at 1.00atm when temperature and number…

Q: A sample of gas contains 0.1700 mol of N2(g) and 0.5100 mol of H2(g) and occupies a volume of 22.6…

A: Nitrogen reacts with hydrogen to form ammonia. The equation for the balanced chemical reaction is…

Q: At 25.0 ° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.60 moles of Gas B. What is…

A: According to the ideal gas law, we know that  PV = nRT Where  P = pressure of the gas V = volume of…

Q: A gas with a mass of 95.14g occupies 48.8L at 659mmHg and 25.3°C. What is its molecular weight? Use…

A:

Q: Consider this molecular-level representation of a mixture of gases. If the partial pressure of the…

A: Relation between partial pressure (Pi) of ith gas, mole fraction of  ith gas (Xi) and total press…

Q: A 0.108g sample of gas at 0.1013 atm and 100 degrees celsius has a volume of 0.240 L. Calculate the…

A:

Q: The volume of a gas at 27.0C and 0.200atm is 80.0mL. What volume will the same gas sample occupy at…

A: Given, Initially, Pressure (P1) = 0.200 atm Volume (V1) = 80.0 mL = 0.08 L Temperature (T1) = 27°C =…

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: 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: The density of 1.00 mol of an unknown gas at a temperature of -71oC and a pressure of 2,359 torr is…

A:

Q: What volume is required to contain 0.045 moles of nitrogen gas under 0.850 atm while at a…

A: For the Nitrogen gas : Temperature, T = 35°C                          = (35 + 273.15) K…

Q: At 25.0 ° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.10 moles of Gas B. What is…

A:

Q: A flask with a volume of 3.17 L contains 9.33 grams of an unknown gas at 32.0°C and 1.00 atm. What…

A:

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: At 25.0° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 5.00 moles of Gas B. What is the…

A: According to ideal gas law PV = nRT where P = total pressure V = volume of vessel n = total moles R…

Q: The density of 1.00 mol of an unknown gas at a temperature of -55°C and a pressure of 2,017 torr is…

A:

Q: At 35.0 °C, a 12.00 L vessel is filled with 6.00 atm of Gas A and 6.89 atm of Gas B. What is the…

A: Given data is as follows: The volume of vessel = 12.00 L The temperature of the system = 35.0 °C The…

Q: Calculate the molar mass of a gas that has a density of 2.5G/L exerts a pressure of 1.75 atm at 55…

A: molar mass = 38.47 g/Mole

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: At 25.0 ° C, a 10.00 L vessel is filled with 5.96 atm of Gas A and 7.89 atm of Gas B. What is the…

A: Assuming Gas A and Gas B to be ideal, we have  PxV=nxRxT where P is  pressure of the gases,  V is…

Q: A large balloon is initially filled to a volume of 25.0L at 353K and a pressure of 2575 mm Hg. The…

A: According to gas equation p1v1/t1=p2v2/t2 V2=p1v1t2/pti

Q: Some N, gas is mixed with some 0, gas, and the sketch below shows a representative sample of the…

A: The ratio of number of molecules of a particular component to the total number of moles is known as…

Q: At 1.00 atm and 4.67 °C, a 2.72 g sample of gas occupies a volume of 1540 mL. Calculate the molar…

A: Given - - > P = 1 atm T =4.67 °C = 277.82 K V=1540 ml =1.54 L m = 2.72 g R = 0.08206…

Q: A gas initially at 5.32 L, 1.69 atm, and 61 °C undergoes a change so that its final volume and…

A:

Q: Consider this molecular-level representation of a mixture of gases. If the partial pressure of the…

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

Q: If 8.0 grams of a gas occupies 22.4 L at 0 °C and 0.25 atm, then the molecular weight of the gas is…

A: By apply ideal gas equation PV=nRTn(no. of moles) = mM= Mass of gasMolar mass of Gas…

Q: An unknown gas at 41.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior,…

A: An unknown gas at 41.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior,…

Q: Consider this molecular-level representation of a mixture of gases. If the partial pressure of the…

A:

Q: A 7.00 L tank at 28.5 °C is filled with 2.61g of carbon monoxide gas and 18.4 g of sulfur…

A: Given- Volume = 7.00 L T = 28.5°C = 28.5 + 273 = 301.5 K Weight of CO = 2.61 gm Weight of SF4 = 18.4…

Q: 7. 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: The values are given as follows:

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

A:

Q: 10. Calculate the partial pressure of each gas, and the total pressure of all gases, if 8.00 grams…

A: Calculate the mole fractions of Ne and Ar,XNe = nNenNe+nAr    ;    XAr = nArnAr + nNe    And then…

Q: Consider this molecular-level representation of a mixture of gases. If the partial pressure of the…

A: The given figure has three types of particles, single blue, single orange and double green. The…

Q: Determine the volume (in L) of 0.25 mol of gas at 545 mmHg and 15oC

A:

Q: If I initially have a gas at a pressure of 14 atm, a volume of 33 Liters, and a temperature of 401…

A: Given: Initial pressure (P1) = 14 atm Initial volume (V1) = 33 L  initial temperature (T1) = 401 K…

Q: Determine the molar mass of an unknown gas if a sample of this gas weighing 0.597 g occupies 100 mL…

A:

Q: At 45.0 °C, a 14.00 L vessel is filled with 7.00 atm of Gas A and 5.89 atm of Gas B. What is the…

A: Given: Partial pressure of gas A = 7.00 atm. And partial pressure of gas B = 5.89 atm.

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

A:

Q: A 3.85 g sample of an unknown gas at 73 °C and 1.05 atm is stored in a 1.35 L flask. What is the…

A:

Q: An unknown gas has a density of .355g/L at 17 celsius and 189mm Hg. Calculate the molar mass of the…

A: Since density = mass / volume  Hence mass of gas = density X volume = 0.355 V hence moles of gas =…

Q: At 1.041.04 atm and 6.78 ∘C6.78⁢ ∘C, a 3.543.54 g sample of gas occupies a volume of…

A:

Q: An empty glass bulb has a volume of 350. mL and a mass of 82.561 g. When filled with an unknown gas…

A: The molar mass of unknown gas filled in in a 350 mL of glass bulb is to be determined from the given…

UV Visible Spectroscopy

Spectroscopy refers to the absorption or emission of light or other radiations by matter. When a substance or chemical absorbs light or radiation, they reach an excited state followed by de-excitation or emission of the light or radiation forming distinct spectra. UV-visible spectroscopy or  ultraviolet-visible refers to the absorption and emission in the ultraviolet and visible regions of the electromagnetic spectrum.