Suppose 0.500 moles of tungsten hexafluoride gas reacts with 1.500 moles of hydr

Question

Suppose 0.500 moles of tungsten hexafluoride gas reacts with 1.500 moles of hydrogen gas with a total pressure of 2.21 atm at 400.00 degrees c in a 50.0 L deposition chamber to form tirgsten metal and hydrogen fluoride gas, Which are then cooled to 0.00 degrees c. What is the final pressure? WF_6(g) + 3H_2(g) rightarrow W(s) + 6 HF(g) A sample of nitrogen gas has a volume of 20.0 L. at 2.00 atm and 35.0 degrees C. If the pressure is increased to 5.00 atm and the temperature decreases to 25.0 degrees C. what volume does the gas occupy? 0.00218 L 11.2 L 8.27 L 7.74 1. 459 L A sample of hydrogen gas at 4.0 atm and 25.0 ml. is heated from 25 degrees C to 40 degrees C. If the pressure remains constant, what is the final volume of the gas? 26.3 mL 105 mL 40.0 mL 25.0 mL 23.8 mL A sample of neon gas al 745 torT and 60.0 L is compressed to 20.0 L. If the temperature remains constant, what is the final pressure of the gas? 2235 torr 761 torr 792 torr 180 torr 3080 torr

Explanation / Answer

22) The reaction stochiometry shows that one mole of tungsten flouride will react with three moles of H2 to give 6 moles of HF gas

So here 0.5 moles of WF6 will react with 1.5 moles of H2 to give 3 moles of HF gas

Pressure = ?

Tempearture = 273.15 K

R = Gas constant = 0.0821 L atm / K mole

V = 50L

We will use ideal gas equation

PV = nRT

P = 3 X 0.0821 x 273.15 / 50

Pressure = 1.35 atm

23) We will use ideal gas equation again.

Intially , Pressure = P1 = 2 atm

Volume = V1 = 20 L

Tempearture = T1 = 35 C = 273.15 + 35 = 308.15 K

Number of moles are same

Finaly

Pressure = P2 = 5 atm

Temperature = T2 = 25 C = 298.15 K

V2 = ?

P1V1 / T1 = P2V2 / T2

V2 = P1 X V1 X T2 / P2 X T1

V2 = 2 X 20 X 308.15 / 5 X 298.15

V2 = 8.268 L = 8.27 L

24) Here pressure and moles are constant, so we will use

V1/ T1 = V2 / T2

V1 = 25mL

T1 = 25 C = 298.15 K

V2= ?

T2 = 40C = 313.15 K

V2 = V1 X T2 / T1 = 25 X 313.5 / 298.15 = 26.257 mL = 26.3 mL

25) Here the number of moles of gas and temperature are constant

so we will use following relation

P1V1 = P2V2

P1 = 745 Torr   V1 = 60 L

P2 = ?            V2 = 20L

P2 = P1V1 / V2 = 745 X 60 / 20 = 2235 Torr

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