|char E1A.11(a) A vessel of volume 22.4 dm’ contains 2.0 mol H,(g) and 1.0 mol P/ ´N,(g) at 273.15K. Calculate (i) the mole fractions of each component, (ii) their partial pressures, and (iii) their total pressure. C E1A 11/h) A .wannal af---

5.31 A McLeod gauge measures low gas pressures by com- pressing a known volume of the gas at constant temperature. If 345 cm' of gas is compressed to a volume of 0.0457. cm' under a pressure of 2.5 kPa, what was the original gns pressure?

A vessel of volume 22.4 dm3 contains 2.0 mol H2(g) and 1.0 mol N2(g) at 273.15 K. Calculate (i) the mole fractions of each component, (ii) their partial pressures, and (iii) their total pressure.

An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2.Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2. V2 = Now, suppose that the above experiment generated n mol of H2(g), that T2 = 0 °C and that P2 = 1 atm. Give the simple algebraic expression, in terms of V2 and n, which equates to the molar volume of H2(g) at STP.VM = 8.829×10-4 mol of B2H6(g) (diborane gas) is generated into a 176.0 mL headspace, at 25.0 °C, thus increasing the pressure by 0.1209 atm. If we assume that the diborane gas obeys Boyle's Law and Charle's Law, what…

For ethane, Pc = 48.2 atm and Tc = 305.4 K. Calculate the pressure exerted by 74.8 g of C2H6 in a 200-cm3 vessel at 37.5°C using (a) the ideal-gas law; (b) the van der Waals equation; (c) the Redlich-Kwong equation; (d) the virial equation, given that for ethane B = -179 cm3/mol and C= 10400 cm6/mol2 at 30°C, and B = -157 cm3/mol and C = 9650 cm6/mol2 at 50°C.

After 1.60 mol of NH3 gas is placed in a 1600-cm3 box at 25 Celcius, the box is heated to 500 K. At this temperature, the ammonia is partially decomposed to N2 and H2 and a pressure measurement gives 4.85 MPa. Find the number of moles of each component present at 500 K.

13. (a) - Calculate the pressure of Xe gas using the ideal gas law and the van der Waals equation of state first at a temperature of 30.0°C and a molar volume of 0.200 L mol-¹ and secondly at a temperature of 500°C and a molar volume of 0.200 L mol-¹ (Note: for Xe a = 4.192 dmº bar mol-2 and b = 0.0516 dm³ mol-¹) ]For each set of conditions in part (a), calculate the % deviation from the ideal (b) pressure. 1 (c) [ intermolecular Explain the deviation from ideality for each set of conditions in terms of forces, temperature, and the effect of the size of the Xe atoms as appropriate.

Please don't provide handwritten solution .....

An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2.Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2.

1.Which incorrect assumptions about gases are corrected by a and b in the van der Waals equation? 2.Use the values of a and b in the table below and the van der Waals equation to calculate the real pressure of 2.55 moles of methane in a cylinder of volume 150.0 mL at a temperature of 332 K.