***** Calculate the volume of each of the following gases at STP. (a)  0.125 g of helium, He               (b)  10.1 g of nitrogen, N2

Carbon dioxide gas at 300 K and 100 kPa is saturated with water vapour. The vapour pressure of water at 300 K is 3.56 kPa. Calculate The amount of vapour in kilograms per m3 of the mixture ?

Calculate the pressure inside a 61.19 L tank containing 1 kg of an equimolar mixture of ethane (1)/propylene (2) at 25 °C. Use the following methods: 1.Ideal Gas Equation 2.Redlick-Kwong EOS Component       X i         Tci(K).    Pci(Pa).        MW Ethane.             0.5.         305.4   4883865    30.07 Propylene.        0.5           365      4620420     42.08

i need the answer quickly

Round off answers to 4 decimal places

1. The Helmholtz function of a certain gas is given by (V – F (T,V) = –nRT |1+ ln v – nb)T? an? пф V where n is the number of moles of gas, T is the temperatures of the gas, V is the volume of the gas, and a, b, and o are constants. (a) Derive the equation of state, the entropy, and the internal energy of the gas. (b) Suppose that 100 moles of the gas expands from 2 m3 to 5 m³ at 280 K and that the constants have the values a = 0.364 J m3 mol-2, b = 4.27 × 10-5 m³ mol-1, and $ = 1.09 × 10-5 m³ K³/2 mol-1. Calculate: (i) AU. (ii) the maximum energy that can be made available for work due to the process.

Show complete solution.Round everything to four decimal places and box all final answers. No units, no points.

PHYSICAL CHEMISTRY:Calculate the pressure exerted by 1.0 mol C2H6 at 1000 K in 100 cm3 using (a) the ideal gas equation and (b) the van der Waals equation. The van der Waals constant for C2H6 are: a = 5.562 bar dm6 mol-2 ; b = 0.06380 dm3 mol-1 answer:[831; 1.72 x 10-3]

In a Van Der Waals gas if the internal energy is given by: u = c,T – a/v, where a is constant. Determine Cy - Cp. Useful information: Cp - C, = [)T + P}()P de а. (Re)*T RT+2a(v-b) (Ru) Tv 1+2a(t-b) (Ro) To RT-2a(v-b) b. с. (Ru) Tv 1-2a(v-b) d.

1. Calculate AU, AH, q, and w for the reversible isothermal expansion of 62.4 g of Ar from a volume of 2.50 L to 15.5 L at 150.0 K. a. Treat Ar as an ideal gas. b. Treat Ar as a gas with the equation of state given below where a represents the van der Waals attraction constant. (We are ignoring the constant b in this problem.) а (P+ -)V = RT V? m т c. Explain any difference between your answers to parts a and b.