ENERGY BALANCES

ON REACTIVE

PROCESS

KHAIRUN NIESA BT ABDULLAH

MOHAMAD AFIQ TRASH CAN HUSIN

RIDUAN BIN HAMID

FARHANA 'ATIQAH BT YUSRI

MASTURA BT MOHIDDIN

NURUL AMIRA SHAQINAH BT MOHD SAIFUL

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HEATS OF REACTION

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Warmth of reaction = sum of heat that needs to be added

or perhaps removed within a chemical reaction.

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Enthalpy sama dengan amount of warmth content employed or on sale since

a system by constant pressure.

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Enthalpy is portrayed as the change in enthalpy.

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The change in enthalpy is related to an alteration in inner

energy (U) and an alteration in the quantity (V), which is

multiplied by constant pressure of the system.

Heat of reaction could be calculated by heat of

formation data.

 ΔHr = (Σ ΔHf of products) – (Σ ΔHf of reactants)

О”H andВ О”HВєrxn

п‚ћ

Δ = presents the enhancements made on the enthalpy; (ΔHproducts ΔHreactants) › a positive worth indicates the products have

greater enthalpy, or perhaps that it is a great endothermic

response (heat is definitely required)

› a negative worth indicates the reactants possess

greater enthalpy, or it is an exothermic

reaction (heat is produced)

п‚ћ

Internal energy of reaction, ∆U r

пѓј

Internal energy occur when the reaction happens

in a sealed reactor by constant quantity.

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∆U r = ∆H l – RT( ∑gas product│vi │- ∑ gas reactnt │vi │)

MEASUREMENT AND

CALCULATION OF HEAT OF

REACTION-HESS LAW

You will discover two ways to calculate ∆ H (enthalpy):

п‚ћ Simply by experimentally(using calorimeter)

п‚ћ By numerically

ΔHº= ∑∆vp∆ HfӨ(products) - ∑∆ vr∆ HfӨ(reactants) Where:

п‚ћ Vp = stoichiometric agent of the item

from the well balanced reaction

п‚ћ Vr = stoichiometric coefficient of the reactant

from the well-balanced reaction

 ∆ Hof = common enthalpy of formation intended for the

reactants or the goods

HESS'S LAW

EXAMPLE:

Determine the value of ∆Ho for the reaction:

2 S i9000 (g) + 2 OF2 (g)

SO2 (g) + SF4 (g)

When

OF2 (g) + H2O(l)

UNITED KINGDOM (g) + 2HF(g) ∆Ho = -277 kJ

SF4 (g) + 2 H2O (l)

SO2(g) + 4HF(g)

∆Ho sama dengan -828 kJ

S(g) + O2 (g)

SO2 (g)

∆Ho = -297 kJ

SOLUTION:

( OF2 (g) + WATER (l)

(SF4 (g) & 2 H2O(l)

( S(g) + T-MOBILE (g )

O2 (g) + 2HF(g) ∆Ho = -277 kJ ) x 2

SO2 (g) & 4HF(g) ∆Ho = -828 kJ ) FLIP

SO2 (g)

∆Ho = -297 kJ ) x 2

2 OF2 (g) +2H2O (l)

two O2 (g) + some HF (g)

SO2 (g) + 4HF (g)

SF4 (g) & 2 H2O (l)

two S (g) + two O2 (g)

2 SO2 (g)

2 S (g) + 2 OF2

SO2 (g) + SF4 (g)

∆Ho sama dengan -277 kJ x a couple of

= -554 kJ

∆Ho = -828 kJ

+ 828 kJ

∆Ho sama dengan -297 kJ x 2 = -594 kJ

∆Ho = -320 kJ

FORMATION REACTION AND HEAT OF

FORMATION

пЃ¶

Formation reactions are chemical reactions that

form one skin mole of element from its component

elements within their standard says.

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Warmth formation sama dengan the measure of energy produced

or consumed when one mole of substance in

standard state ( 1atm and 298. 15 K ) is created from

the pure factors under the same conditions

пЃ¶

О”HВ° sama dengan ОЈ(ОЅ Г— О”HfВ°) (products) - ОЈ(ОЅ Г— О”HfВ°) (reactants)

METHODS FOR THE

CALCULATION OF ONE'S

BALANCES

Attract and packaging a flowchart

HEAT OF COMBUSTION

п‚ћ

Standard temperature of combustable of a subtance О”HВ°c can be

the heat of combustion of these subtance with oxygen

to yield specified products in standard condition(25C

and you atm )

п‚ћ

ΔH°C = Ƹ[ΔH°c (reactants) ] –

Жё[О”HВ°c(products)]

PASS 12 MONTHS EXAMINATION

QUESTION(JUNE 2014)

п‚ћ

The standard temperature of reaction

C2H4(g) + 2 CI2(g)

C2HCI3(l)+H2(g)

+HCI(g) is

∆H r sama dengan -420. 8kJ/mol. Calculate ∆U r with this

reaction.