Question

Information:

In this experiment, you will fill a gelatin capsule with an alloy sample. If the mass of the gelatin capsule is 0.123 g, and the mass of the capsule plus alloy sample is 0.215 g, calculate the mass, in grams, of the alloy sample. - 0.092 g
The alloy sample is dissolved in HCl and H₂ gas is produced and collected over water. The volume of H₂ gas produced is 89.5 mL. What is the volume of gas, in liters? - 0.0895 L

The temperature of the water is 24.0 ^oC. What is the temperature in Kelvin? T(K) = T(^oC) + 273.15 - 297.15

A. The barometric pressure is 766.1 mmHg. The vapor pressure of water at 24.0 C is 22.4 mmHg. Calculate the pressure, in mmHg, of the dry hydrogen gas.

B. Convert the pressure of the dry H2 to units of atm. 760.0 mm Hg = 1 atm.

C. Calculate moles of H2 produced in the reaction. R = 0.08206 L atm/(mol K)

Answer 1

A .

According to dalton's law total pressure of gas is equal to sum of partial pressure exerted by each individual gas

P_total = P₁ + P₂

P_H2 = P_total - P_{water vapour}

P_H2 = 766.1 - 22.4 = 743.7 mmHg

Pressure of dry hydrogen gas = 743.7 mmHg

B.

760.0 mmHg = 1 atm then 743.7 mmHg = 743.7 X 1 / 760 = 0.97855 atm

743.7 mmHg = 0.97855 atm

C.

Use ideal gas equation for calculation of mole of gas

Ideal gas equation

PV = nRT             where, P = atm pressure= 0.97855 atm,

V = volume in Liter = 89.5 ml = 0.0895 L

n = number of mole = ?

R = 0.08206L atm mol^-1 K^-1 =Proportionality constant = gas constant,

T = Temperature in K = 297.15 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.97855X 0.0895) / (0.08206X 297.15) = 0.00359 mole

mole of H₂ produced in reaction = 0.00359 mole