Chapter 5, Problem 125AE

Interpretation Introduction

Interpretation:

The partial pressure of hydrogen gas in the sample should be calculated and the mass of zinc in grams which is reacted to produce this quantity of hydrogen.

  $\text{Zn(s)+2HCl(aq)}\to {\text{ZnCl}}_{\text{2}}{\text{(aq)+H}}_{\text{2}}\text{(g)}$

Concept Introduction:

Mole is SI unit which is used to measure the quantity of the substance. It is the quantity of a substance which contains same number of atoms as present in accurately 12.00 g of carbon-12 is known as mole.

Number of moles of a compound is defined as the ratio of given mass of the compound to the molar or molecular mass of the compound.

The mathematical expression is given by:

Number of moles = $\frac{\text{given mass of the compound}}{\text{molar mass of the compound}}$

Idea gas equation is:

  $\text{PV= nRT}$

Where,

P = pressure

V = volume

n = number of moles

R = universal gas constant

T = temperature

Dalton’s Law of partial pressure is used for calculating the total pressure of a mixture of gases.

It states that, in a mixture of two or more gases, the total pressure is equal to the sum of the partial pressures of individual gases.

The mathematical expression is:

  $P_{total}=P_1+P_2+P_3+P_4+\mathrm{........}$

The partial pressure of a gas is equal to the product of total pressure and mole fraction of a gas.

The mathematical expression is:

  $P={\chi }_A{P}_{total}$

Where, P = pressure of a gas

  ${\chi }_A$ = mole fraction

  $P_{Total}$ = Total pressure