Chapter 5, Problem 5.102P

(a)

Interpretation Introduction

Interpretation:

The volume of carbon dioxide which is produced from 20.0 g of glucose and excess oxygen gas should be calculated when the reaction occur in expandable container at $37°C$ and 780 torr.

  ${\mathrm{C}}_6{H}_{12}{O}_6{\text{(s) + 6O}}_2(\text{g})\to 6{\text{CO}}_{\text{2}}{\text{(g) + 6H}}_2\text{O(g)}$

Concept Introduction:

Ideal gas law equation is shown as:

  $\text{PV= nRT}$

Where,

P = Pressure

V = Volume

n = Number of moles

R = Universal gas constant

T = Temperature

Rearrange the above formula in terms of volume:

  $V=\frac{nRT}{P}$

Number of moles is defined as the ratio of mass to the molar mass.

The mathematical expression is given as:

  $\text{Number of moles =}\frac{\text{Mass}}{\text{Molar mass}}$

(b)

Interpretation Introduction

Interpretation:

The partial pressure of every gas should be calculated when the reaction is 50% complete that is 10.0 g of glucose left.

  ${\mathrm{C}}_6{H}_{12}{O}_6{\text{(s) + 6O}}_2(\text{g})\to 6{\text{CO}}_{\text{2}}{\text{(g) + 6H}}_2\text{O(g)}$

Concept Introduction:

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:

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