1) what volume will 300 ml of gas at 20 C and a pressure of355 mmHg occupy if th
ID: 688845 • Letter: 1
Question
1) what volume will 300 ml of gas at 20 C and a pressure of355 mmHg occupy if the temperature is reduced to -80C and thepressure increased to 760mmHg? 2) a sample of gas of mass 2.82 g occupies a volume of 639 mlat 27 C and 1.00 atm pressure. what is the molar mass of thegas? 1) what volume will 300 ml of gas at 20 C and a pressure of355 mmHg occupy if the temperature is reduced to -80C and thepressure increased to 760mmHg? 2) a sample of gas of mass 2.82 g occupies a volume of 639 mlat 27 C and 1.00 atm pressure. what is the molar mass of thegas?Explanation / Answer
a) Use the equation PV=nRT Solve the equation for the unknowns (P, V, and T) You get with the variables ----> (P1V1 / T1)=(R2V2 / T2) Convert mm Hg to atm ---> P1 = 0.4671232 atm and P2 = 1.0000384atm Convert C to K ---> T1 = 293.15 K and T2 = 193.15 K Convert mL to L ---> V1 = 0.3 L Next, plug in the values and solve for V2 ((0.4671232 atm)(0.3 L) / 293.15 K) = ((1.0000384 atm)(V2) / 193.15K) V2 = 0.092329574 L or 0.0923 L b) this time i just went ahead and did the conversions to theproper units. You need to use PV=nRT again to solve for n (# of moles). R is the constant 0.082057 (1 atm) (0.639 L) = n (0.082057) (300.15 k) n = 0.025944594 mols Molar mass = (grams / mol ) (2.82 g / 0.025944594 mols) = Molar mass of the gas = 108.6931645or 108.7 g / mol Hope this helps. P:EASE RATE!!!!
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