Show work and answer problems A 0210 gram sample of a metal

A 0.210 gram sample of a metal, M, reacts completely with sulfuric acid according to: A volume of 219 mL of hydrogen is collected over water; the water level in the co as the outside level. Atmospheric pressure is 7560 Torr and the temperature is 25 . The vapor pressure of water at various temperatures can be found in this table, Calculate the molar mass of the metal. vessel is the same Number g/mol about us careers1 privacy pelicy j 3 4 5 6 8 9 0

Solution

Use the ideal gas equation to calculate mole of H₂ formed

vapur pressure water at 25⁰C = 23.8 torr

PV = nRT             where, P = atm pressure= 756 - 23.8 torr = 732.2 torr = 0.9634 atm,

V = volume in Liter = 219 ml = 0.219 L

n = number of mole = ?

R = 0.08205L atm mol^-1 K^-1 =Proportionality constant = gas constant,

T = Temperature in K = 25⁰C = 273.15+ 25 = 298.15 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.9634X 0.219)/(0.08205 X 298.15) = 0.008625 mole

0.008625 mole H₂ gas produced

According to reaction to produce 1 mole H₂ required metal is 1 mole therefore to produce 0.008625 mole H₂ required metal is 0.008625 mole

thus 0.210 gm metal = 0.008625 mole metal therefore 1 mole metal = 0.210 X1 / 0.008625 = 24.35

molar mass of metal = 24.35 g/mol