A3.60 l gas sample is at a pressure of 95.5 kpa and a temperature of 25.0°c. if the gas sample weighs 6.10 g, calculate the molar mass of the gas.

Strategy of solution:

First, find the number of moles of the gas using the law pV = nRT. After that, find the molar mass by dividing the mass of the compound by the number of moles: molar mass = n / mm

Solution:

1)
p = 95.5 kPa
T = 25.0 + 273.15 K = 298.15 K
V = 3.60 l
R = 8.314 (l * kPa / K*mol)

=> n = pV / RT = [95.5 kPa * 3.60 l ] / [8.314 (l*kPa/K*mol) * 298.15 K] = 0.139 mol

2) mm = number of grams / number of moles = 6.10 g / 0.139 mol = 43.88 g/mol

43.9 g / mol (rounded to three significant figures)

The activity series is shown in the attached picture. if the element is below the other, then you can displace the other. following the activity series as a guide, the reactions are as follows: nickel and aluminum chloride3 ni + 2 alcl₃  → 3 nicl₂ + 2 albarium and copper bromideba + cubr  →  no reaction because cu is less oxidizable than bapotassium nitrate and aluminum3 kno₃ + al  → al(no₃)₃ + 3 ksodium phosphate and zincnaso₄ + zn  → znso₄ + na