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 1550 kg/h · 50% saltStream 2ṁ₂ = ? · 5% saltProduct10% salt

How much of stream 2 must be added each hour to stream 1 so that the blended product contains 10% salt? Find ṁ2.

ṁ1 = 550 kg/hx1 = 50 %x2 = 5 %x3 = 10 %
ṁ2 = kg/h
2.Mass balanceHard
EvaporatorFeed F900 kg/h · 10% sugarProduct P65% sugarVapour W (pure water)W = ? kg/h

An evaporator concentrates a sugar solution by boiling off pure water. Find the water evaporated W in kg/h.

F = 900 kg/hxF = 10 %xP = 65 %
W = kg/h
3.Energy balanceMedium
hot sidecold sidelight oil · 130 °C70 °Cwater · 30 °Ct = ? °C

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

ṁh = 2 kg/scp,h = 2.1 kJ/(kg·K)Th: 130 → 70 °Cṁc = 1.5 kg/scp,c = 4.18 kJ/(kg·K)tin = 30 °C
tout = °C
4.Energy balanceHard
hot sidecold sideglycol mix · 120 °C70 °Cwater · 10 °C80 °C · ṁ = ?5% lost

Hot glycol mix heats water in an exchanger that loses 5% of the heat released by the hot stream to the surroundings. Find the water flow rate ṁc needed.

ṁh = 2 kg/scp,h = 3.6 kJ/(kg·K)Th: 120 → 70 °Ct: 10 → 80 °Ccp,c = 4.18 kJ/(kg·K)loss = 5 %
ṁc = kg/s
5.Ideal gas lawMedium
470 g of N₂V = 20 LT = 0 °CP = ?

A tank of 20 L contains 470 g of N₂ at 0 °C. Treat it as an ideal gas and find the pressure P.

m = 470 gM = 28.01 g/molV = 20 LT = 0 °CR = 8.314 J/(mol·K)
P = kPa
6.Ideal gas lawHard
He, M = 4.003 g/molP = 150 kPaT = 20 °Cρ = ?

Find the density ρ of He at 150 kPa and 20 °C, treating it as an ideal gas.

M = 4.003 g/molP = 150 kPaT = 20 °CR = 8.314 J/(mol·K)
ρ = kg/m³
7.StoichiometryMedium
m(X)n(X)n(CO2​)m(CO2​)÷ M(X)× 1/ν× M(CO2​)

24 g of CH4 and 64 g of O2 react according to CH4 + 2O2 → CO2 + 2H2O. What mass m of CO2 can form?

M(CH4) = 16.04M(O2) = 32M(CO2) = 44.01 g/mol
m = g
8.StoichiometryHard
m(CH4​)n(CH4​)n(H2​O)m(H2​O)÷ M(CH4​)× 2/1× M(H2​O)

In the reaction CH4 + 2O2 → CO2 + 2H2O, 6 g of CH4 reacts completely (the other reactants are in excess) and 12.27 g of H2O is collected. Find the percent yield Y.

M(CH4) = 16.04 g/molM(H2O) = 18.02 g/molactual: 12.27 g
Y = %

3Solutions

1.Mass balance

Answer: ṁ2 = 4400 kg/h

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

Balances

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

Solve for ṁ2

ṁ2 = ṁ1(x1 − x3)/(x3 − x2) = 550·(50 − 10)/(10 − 5) = 4400 kg/h

Answer

ṁ2 = 4400 kg/h
2.Mass balance

Answer: W = 761.5 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 = 900·10/65 = 138.5 kg/h

Total balance

W = F − P = 900 − 138.5 = 761.5 kg/h

Answer

W = 761.5 kg/h
3.Energy balance

Answer: tout = 70.19 °C

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

Heat released by the hot stream

Q = 2·2.1·(130 − 70) = 252 kW

Heat picked up by the water

tout = tin + Q/(ṁccp,c) = 30 + 252/(1.5·4.18) = 70.19 °C

Answer

tout = 70.19 °C
4.Energy balance

Answer: ṁc = 1.169 kg/s

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

Heat released

Qh = 2·3.6·(120 − 70) = 360 kW

Heat that reaches the water

Qc = (1 − 0.05)·360 = 342 kW

Water flow rate

ṁc = Qc/(cp,c·Δt) = 342/(4.18·70) = 1.169 kg/s

Answer

ṁc = 1.169 kg/s
5.Ideal gas law

Answer: P = 1905 kPa

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

Moles

n = m/M = 470/28.01 = 16.78 mol
T = 0 + 273.15 = 273.1 K

Pressure

P = nRT/V = 16.78·8.314·273.1/0.02 = 1905 kPa

Answer

P = 1905 kPa
6.Ideal gas law

Answer: ρ = 0.2464 kg/m³

Ideal gas density: ρ = PM/(RT).

Rearrange the gas law

PV = (m/M)RT → ρ = m/V = PM/(RT)
T = 20 + 273.15 = 293.1 K

Density

ρ = 150·4.003/(8.314·293.1) = 0.2464 kg/m³

Answer

ρ = 0.2464 kg/m³
7.Stoichiometry

Answer: m = 44.01 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(CH4) = 24/16.04 = 1.496 mol
n(O2) = 64/32 = 2 mol

Limiting reactant

1.496/1 = 1.496, 2/2 = 1 → O2

Mass of product

n(CO2) = 1·1 = 1 mol
m = 1·44.01 = 44.01 g

Answer

m = 44.01 g
8.Stoichiometry

Answer: Y = 91.01 %

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(CH4) = 6/16.04 = 0.3741 mol
m = 0.3741·2/1·18.02 = 13.48 g

Percent yield

Y = 12.27/13.48·100 = 91.01%

Answer

Y = 91.01%

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