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- .....................An 85 g-mol gas 0ccupies 38 L at 78oC,,, wh@t is the vacuum pressure 0f the gas in psi??? CH0iceS: 210.4421 195.7421 -195.742 225.1421 961.6895 946.9895 932.2895 -932.289A 500.0 mL sealed canister only containing exactly 0.1376 mol of n-pentane (CH3CH2CH2CH2CH3) is heated to 350.0 °C.All of the n-pentane will have vapourized.Use Van der Waal's equation to calculate the pressure.(Pobs+[(n2a)/(V2)])(V−nb)=nRTFor n-pentane: a=19.01 L2 atm/mol2; b=0.146 L/mol. P(obs)=Aflask_with a v0lume 0f3.16L c0ntains 8g 0f an unkn0wnGas at32oC and 1atm. What is the m0larmass (g/m0l) 0f the gas?
- A 500.0 mL sealed canister only containing exactly 0.1209 mol of methylamine (CH3NH2) is heated to 330.0 °C.All of the methylamine will have vapourized.Use Van der Waal's equation to calculate the pressure.(Pobs+[(n2a)/(V2)])(V−nb)=nRTFor methylamine: a=7.13 L2 atm/mol2; b=0.05992 L/mol.desired Mg mass =0.0340g "Atmospheric pressure (mmHg): 733.59Trial 1 and Trial 2 values separated by commas:Mass of Mg (g): 0.038, 0.031Temperature (°C): 20.2 (both trials)Vapor pressure of water (mmHg): 17.86 (both trials)Volume of gas (mL): 42.95, 35.80 need calculations for table.A sealed cubical container 21.0 cm on a side contains a gas with five times Avogadro's number of argon atoms at a temperature of 30.0°C. HINT (a) Find the internal energy (in J) of the gas. J (b) The total translational kinetic energy (in J) of the gas. J (c) Calculate the average kinetic energy (in J) per atom. J (d) Use P = 2 3 N V 1 2 mv2 to calculate the gas pressure (in Pa). Pa (e) Calculate the gas pressure (in Pa) using the ideal gas law (PV = nRT). Pa
- The molar mass of Freon-11 gas sample weighing 0.597 g and occupies 100 mL at 95oC and 1.32 atm. is: (R=0.082 L atm/Kmole)The following system is used for q7-q9 10.00g of O2 and 15.00g N2 are combined in a 20.0L container at 25.00oC O2 32.00g/mol N2 28.02 g/mol R= 0.08206 L atm/mol K What is the total pressure (atm) in the system above? Answer to 3 sig figs1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.
- A glass container was initially charged with 2.60 moles of a gas sample at 3.75 bar and 21.7 C. some of the gas was released as the temperature was increased to 28.5 C, so the final pressure in the container was reduced to 0.998 bar. how many moles of the gas sample are present at the end?Pressure (P) Volume (V) Temperature (T) Moles (n) 1. 5.00 atm 25.00 L 273.15 K 2. 0.55 L 308 K 0.50 mol 3. 20.00 atm 30.00 L 25.30 mol 4. 15.00 atm 370.00 K 3.00 mol 5. 10.50 L 280.00 K 10.00 molIdeal Gas Law 13. a) How many moles of CO2 gas occupy a volume of 757 mL at 10.4 atm and 317Kelvin? b. How many grams of CO2 gas are present? please make sure final answers are in sig figs