Reference no: EM133025061

Mass And Energy Balance

FUNDAMENTAL PRINCIPLES

Question 1. (a) State what the following terms represent and give an example of where each may be used:
(i) w/w
(ii) w/v
(iii) v/v(iv) mole fraction
(v) mass fraction.
(b) What is the difference between the units 'kmol' and 'mol'?
(c) (i) Name the three main ideal gas laws and give the mathematical way of expressing each.
(ii) How are they combined in a single equation?
(iii) Use the ideal gas laws to calculate the mass of 25 m³ of a mixture of 21% v/v oxygen (O₂) and 79% nitrogen (N₂) which is at a temperature of 65°C and pressure of 2 bar.

Question 2. For each of the following compounds:
(i) aluminium chloride - AlCl₃
(ii) iron (III) sulphate (ferric sulphate) - Fe₂(SO₄)₃
(iii) cobalt nitrate - Co(NO₃)₂
(iv) sodium phosphate - Na₃PO₄

(v) amino-butane - C₄H₉NH₂

calculate, using values obtained from the Periodic Table given in Lesson 1: (a) the number of moles of that compound present in a mass of 200 g
(b) the amount in grams per litre (g l-1) contained in a 2 M solution of the compound.

Question 3. (a) Classify the following changes as either physical or chemical:
(i) the melting of ice
(ii) the purification of sugar by dissolving and re-crystallising
(iii) the removal of an acid gas by dissolving it in an alkali solution
(iv) the removal of water and gas from crude oil by settling and then separating the oil by distillation into various fractions (v) converting water into hydrogen and oxygen by electrolysis.
(b) Balance the following chemical equations, if necessary:
(i) MnO₂( )s + HCl(aq) → MnCl₂(aq) + HO₂ (l) + Cl₂( )g
(ii) Zn OH( )2(aq) + H SO₂ 4(aq) → ZnSO₄(aq) + HO₂ (l)
(iii) CHNH₂ 5 2( )l + O₂(g) → CO₂(g) + HO₂ (l) + N₂(g)
(iv) Al(s) + ZnO(s) → Al O₂ 3(s) + Zn(s)
(v) CaO( )s + H O₂ (l) → Ca OH( )2(s)
(c) For each of the following balanced equations, calculate the amounts of each reactant required to produce 100 kg of the product underlined (assume 100% conversion).
(i) H₂(g) + S(l) → H S₂ (g)

(ii) 3NaOH(aq) + H PO3 4(aq) → Na PO3 4(aq) + 3H O2 (l)

(iii) 2C H₂ 6( )g + 7O2(g) → 4CO₂(g) + 6H O₂ (g)

Question 4. Explain the terms:
(a) limiting reactant
(b) excess reactant
(c) tie substances
(d) % conversion
(e) equilibrium
(f) recycle
(g) purge
(h) by-pass.

Question 5. Sulphur trioxide is formed by the reaction between sulphur dioxide and air (more correctly oxygen) in a catalytic reactor, according to the unbalanced equation

SO₂(g) + O₂(g) →catalyst SO₃(g)

The reaction conditions give a 50% conversion when stoichiometric quantities of the reactants are used.
(a) Balance the equation.
(b) Calculate the composition (on a mole fraction basis) of the final mixture leaving the reactor.
Data: air consists of 21% v/v oxygen and 79% v/v nitrogen.

Attachment:- FUNDAMENTAL PRINCIPLES.rar