Question

On a hot summer day, the density of air at atmospheric pressure at 32.5°C is 1.2074 kg/m3. (a) What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? 35.0146 Your response differs from the correct answer by more than 10%. Double check your calculations, mol (b) Avogadro's number of air molecules has a mass of 2.86 x 10-2 kg. What is the mass of 1.00 m3 of air? (Assume air is an ideal gas.) 1.0014 x Your response differs from the correct answer by more than 10%. Double check your calculations. kg (c) Does the value calculated in part (b) agree with the stated density of air at this temperature? (Consider that it does if the values are within 10% of each other.) O Yes Ο Νο

Answer 1

Answers a) pressure P= I atm => 1001 x 10 Pa Temperature T-32.5°C -7 32:5+273 - 30 5.5k Density (= 12074 kg/m3 volume v=1m3 From the relation PUEURT na pusat R has constant -8.314 J/molk n-1.01x105) (1) (8.314 x 305.5) n = 39.76 mol (6) Avogadros number of air moralles has a mass of -2.86X162 kg mslav how 286 xio° 9 The mass of im² of air is m=nM 39.76 x 2.86X102 m=1137 (0) Density of the air lam e 1.137 - T e = 1.137 kg/m3 Percentage difference in density - Pue xlop =1:137-102074x1oo 1.2074 =-5.8 Yes