Material and Energy Balances: cram pack

Formula sheets, the key method steps for every topic and 8 practice problems, with full solutions at the back.

New problemsBack to the course

In the print window, choose “Save as PDF” to keep a copy on your device.

1Formulas and methods

Mass balance

Steady state
in = out
Total balance
ṁ1 + ṁ2 = ṁ3
Component balance
ṁ1x1 + ṁ2x2 = ṁ3x3
Evaporator
F·xF = P·xP, W = F − P

Energy balance

Sensible heat
Q = ṁ·cp·ΔT
Latent heat
Q = ṁ·hfg
Mixing
ΣṁcpTin = ΣṁcpTout
Water
cp ≈ 4.18 kJ/(kg·K)

Ideal gas law

Ideal gas law
pV = nRT
Gas constant
R = 8.314 J/(mol·K)
Combined gas law
p1V1/T1 = p2V2/T2
Moles
n = m/M
Temperature
T[K] = T[°C] + 273.15

Stoichiometry

Moles
n = m/M
Concentration
c = n/V
Mole ratio
use the coefficients of the balanced equation
Limiting reactant
the one that runs out first
Percent yield
actual / theoretical × 100%

Method

  1. Write and balance the chemical equation.
  2. Convert the given mass to moles: n = m/M.
  3. Use the coefficients as the mole ratio to find the moles of the substance you want.
  4. Convert back to mass with m = n·M. With two reactants, find the limiting reactant first.

2Practice problems

1.Mass balanceMedium
MixerStream 1450 kg/h · 50% sugarStream 2ṁ₂ = ? · 10% sugarProduct35% sugar

How much of stream 2 must be added each hour to stream 1 so that the blended product contains 35% sugar? Find ṁ2.

ṁ1 = 450 kg/hx1 = 50 %x2 = 10 %x3 = 35 %
ṁ2 = kg/h
2.Mass balanceHard
EvaporatorFeed F4300 kg/h · 17% NaOHProduct PP = ? · 30%Vapour W (pure water)0% NaOH

An evaporator concentrates a NaOH solution by boiling off pure water. Find the product flow P in kg/h.

F = 4300 kg/hxF = 17 %xP = 30 %
P = kg/h
3.Energy balanceMedium
hot sidecold sideglycol mix · 180 °C150 °Cwater · 20 °Ct = ? °C

Hot glycol mix cools water in a counter-flow heat exchanger with no heat loss. Find the water outlet temperature tout.

ṁh = 3 kg/scp,h = 3.6 kJ/(kg·K)Th: 180 → 150 °Cṁc = 3 kg/scp,c = 4.18 kJ/(kg·K)tin = 20 °C
tout = °C
4.Energy balanceHard
hot sidecold sideethanol · 120 °C70 °Cwater · 25 °C70 °C · ṁ = ?15% lost

Hot ethanol heats water in an exchanger that loses 15% of the heat released by the hot stream to the surroundings. Find the water flow rate ṁc needed.

ṁh = 3 kg/scp,h = 2.44 kJ/(kg·K)Th: 120 → 70 °Ct: 25 → 70 °Ccp,c = 4.18 kJ/(kg·K)loss = 15 %
ṁc = kg/s
5.Ideal gas lawMedium
200 g of N₂V = 5 LT = 15 °CP = ?

A tank of 5 L contains 200 g of N₂ at 15 °C. Treat it as an ideal gas and find the pressure P.

m = 200 gM = 28.01 g/molV = 5 LT = 15 °CR = 8.314 J/(mol·K)
P = kPa
6.Ideal gas lawHard
State 1State 2

A fixed amount of CO₂ goes from 150 kPa, 2 L, 40 °C to 400 kPa and 80 °C. Find the new volume V2.

P1 = 150 kPaV1 = 2 LT1 = 40 °CP2 = 400 kPaT2 = 80 °C
V2 = L
7.StoichiometryMedium
m(X)n(X)n(CO2​)m(CO2​)÷ M(X)× 3/ν× M(CO2​)

12 g of C3H8 and 20 g of O2 react according to C3H8 + 5O2 → 3CO2 + 4H2O. What mass m of CO2 can form?

M(C3H8) = 44.1M(O2) = 32M(CO2) = 44.01 g/mol
m = g
8.StoichiometryHard
m(Mg)n(Mg)n(MgO)m(MgO)÷ M(Mg)× 2/2× M(MgO)

In the reaction 2Mg + O2 → 2MgO, 20 g of Mg reacts completely (the other reactants are in excess) and 20.56 g of MgO is collected. Find the percent yield Y.

M(Mg) = 24.31 g/molM(MgO) = 40.3 g/molactual: 20.56 g
Y = %

3Solutions

1.Mass balance

Answer: ṁ2 = 270 kg/h

Steady-state mass balance: in = out for the total and for each component. Blending problems combine both.

Balances

Total: ṁ3 = ṁ1 + ṁ2
sugar: ṁ1x1 + ṁ2x2 = (ṁ1 + ṁ2)x3

Solve for ṁ2

ṁ2 = ṁ1(x1 − x3)/(x3 − x2) = 450·(50 − 35)/(35 − 10) = 270 kg/h

Answer

ṁ2 = 270 kg/h
2.Mass balance

Answer: P = 2437 kg/h

Tie component: a component that passes through unchanged in one stream (here the solute) links the flows directly. Then the total balance gives the rest.

Solute balance

F·xF = P·xP → P = 4300·17/30 = 2437 kg/h

Answer

P = 2437 kg/h
3.Energy balance

Answer: tout = 45.84 °C

Exchanger energy balance: with no losses, ṁhcp,h(Th,in − Th,out) = ṁccp,c(tout − tin).

Heat released by the hot stream

Q = 3·3.6·(180 − 150) = 324 kW

Heat picked up by the water

tout = tin + Q/(ṁccp,c) = 20 + 324/(3·4.18) = 45.84 °C

Answer

tout = 45.84 °C
4.Energy balance

Answer: ṁc = 1.654 kg/s

Energy balance with losses: heat released = heat absorbed + heat lost.

Heat released

Qh = 3·2.44·(120 − 70) = 366 kW

Heat that reaches the water

Qc = (1 − 0.15)·366 = 311.1 kW

Water flow rate

ṁc = Qc/(cp,c·Δt) = 311.1/(4.18·45) = 1.654 kg/s

Answer

ṁc = 1.654 kg/s
5.Ideal gas law

Answer: P = 3421 kPa

Ideal gas law: PV = nRT, with n = m/M.

Moles

n = m/M = 200/28.01 = 7.14 mol
T = 15 + 273.15 = 288.1 K

Pressure

P = nRT/V = 7.14·8.314·288.1/0.005 = 3421 kPa

Answer

P = 3421 kPa
6.Ideal gas law

Answer: V2 = 0.8458 L

Combined gas law: for a fixed amount of ideal gas, P1V1/T1 = P2V2/T2.

Absolute temperatures

T1 = 313.1 K, T2 = 353.1 K

Combined gas law

V2 = V1·(P1/P2)·(T2/T1) = 2·(150/400)·(353.1/313.1) = 0.8458 L

Answer

V2 = 0.8458 L
7.Stoichiometry

Answer: m = 16.5 g

Stoichiometry: a balanced equation counts particles, not grams. Convert mass to moles with n = m/M, use the coefficients of the equation as the mole ratio, then convert back with m = n·M. With two reactants, the limiting reactant is the one that runs out first and fixes how much product forms.

Moles of each reactant

n(C3H8) = 12/44.1 = 0.2721 mol
n(O2) = 20/32 = 0.625 mol

Limiting reactant

0.2721/1 = 0.2721, 0.625/5 = 0.125 → O2

Mass of product

n(CO2) = 0.125·3 = 0.375 mol
m = 0.375·44.01 = 16.5 g

Answer

m = 16.5 g
8.Stoichiometry

Answer: Y = 62.01 %

Stoichiometry: a balanced equation counts particles, not grams. Convert mass to moles with n = m/M, use the coefficients of the equation as the mole ratio, then convert back with m = n·M. With two reactants, the limiting reactant is the one that runs out first and fixes how much product forms.

Theoretical yield

n(Mg) = 20/24.31 = 0.8227 mol
m = 0.8227·2/2·40.3 = 33.16 g

Percent yield

Y = 20.56/33.16·100 = 62.01%

Answer

Y = 62.01%

ExamProblems · examproblems.com/courses/material-and-energy-balances