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First Law Analysis for Reacting System

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First Law Analysis for Reacting System. Consider a constant pressure process in which n f moles of fuel react with n a moles of air to produce n p moles of product:. Products. Reactants. W. Q. Products. Reactants. State 1. State 2. Reaction.

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slide1

First Law Analysis for Reacting System

Consider a constant pressure process in which nf moles of fuel react with

na moles of air to produce np moles of product:

Products

Reactants

W

Q

Products

Reactants

State 1

State 2

Reaction

Applying First Law with state 1 being the reactants at P1, T1 and state 2

being products at P2, T2:

slide2

First Law Analysis for Reacting System

HP < HRQ< 0 exothermic reaction

HP > HRQ > 0 endothermic reaction

slide3

Enthalpy of Reaction

Consider the case where the final temperature of the products is the same as

the initial temperature of the reactants (e.g., calorimeter is used to measure Q).

W

P1=P2=Po

T1=T2=To

Q

To

Reaction

The heat released under this situation is referred to as the enthalpy of

reaction, DHR ,

slide4

Heat of Combustion

The maximum amount of energy is released from a fuel when reacted with a

stoichiometric amount of air and all the hydrogen and carbon contained in the

fuel is converted to CO2 and H2O

This maximum energy is referred to as the heat of combustion or the heating

value and it is typically given per mass of fuel

DHR(298K)

slide5

T

hf

hg

Tp

S

Heat of Combustion

There are two possible values for the heat of combustion that can be calculated

depending on whether the water in the products is taken to be in a liquid or

vapour state.

From steam tables:

hfg = hg – hf > 0

DHR = HP – HR < 0 (exothermic)

The term higher heat of combustion is used when the water in the products

is taken to be in the liquid state

The term lower heat of combustion is used when the water in the products

is taken to be in the vapour state

slide6

Heat of Formation

Consider the following reactions taking place at atmospheric pressure and

with TP = TR= 298K

In these reactions H2O and CO2 are formed from their elements in their

natural state at standard temperature and pressure (STP) 1 atm and 298K.

Reactions of this type are called formation reactions and the corresponding

measured heat release Q is referred to as the standard heat of formation

and takes the symbol so:

Values for standard heat of formation for different species are tabulated

slide7

Enthalpy Scale for a Reacting System

We need to take into account that for a reacting system the working fluid

changes molecularly from reactants to products while undergoing a process.

Consider the following identity:

By international convention, the enthalpy of every element in its natural state

(e.g., O2(g), N2(g), H2(g), C(s)) at STP has been set to zero

(note the notation convention)

at STP

slide8

Enthalpy Scale for a Reacting System

The enthalpy of all other substances at STP is simply the heat of formation

of the substance, since it is formed from its elements, for example:

Therefore, the enthalpy of the i’th component in a mixture is:

chemical enthalpy

sensible enthalpy

The sensible enthalpy for different species is tabulated as a function of

temperature (JANNAF Tables).

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