a) A burette which contains 0.001 moles of Mg metal and HCl solution, was invert

Question

a) A burette which contains 0.001 moles of Mg metal and HCl solution, was inverted in water bath of 300 kelvin. The reaction produces 0.025 L of hydrogen gas with a total pressure of 1 atm. Calculate the gas constant of H2.

b) A 0.614 mole sample of ideal gas at 12 °C occupies a volume of 4.3 L. What is the pressure of the gas? (R = 0.0821 L.atm/mol.K)

c) Determine the volume occupied by 0.001 moles of H2 gas at a temperature of 298K and a pressure of 1 atm. (R = 0.0821 L.atm/mol.K)

d) A sample of H2 gas, at a temperature of 303K and a pressure of 1 atm, occupies 22.2 liters. Determine the mass of H2 gas. (molar mass of H = 1) (R = 0.0821 L.atm/mol.K)

Explanation / Answer

a)

PV = nRT

R = PV/(nT)

R = (1)(0.025)/(0.001*300)

R = 0.083333

b)

Aply

PV = nRT

P = nRT/V

P = 0.614*0.082*(12+273)/(4.3)

P = 3.3370186 atm

c)

V = nRT/P

V = (0.001)(0.082)(298)/(1) = 0.024436 L

d)

Find

n = PV/(RT)

n = (1*22.2)/(0.0.82*303)

n = 0.893503

mass = mol*MW = 0.893503*2 = 1.787006 g of H2

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