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BlackZzzverrR [31]
3 years ago
9

Calculate the value of K p for the equation C ( s ) + CO 2 ( g ) − ⇀ ↽ − 2 CO ( g ) K p = ? given that at a certain temperature

C ( s ) + 2 H 2 O ( g ) − ⇀ ↽ − CO 2 ( g ) + 2 H 2 ( g ) K p 1 = 3.09 a t m H 2 ( g ) + CO 2 ( g ) − ⇀ ↽ − H 2 O ( g ) + CO ( g ) K p 2 = 0.793
Chemistry
1 answer:
kogti [31]3 years ago
5 0

<u>Answer:</u> The value of K_p for the net reaction is 1.94

<u>Explanation:</u>

The given chemical equations follows:

<u>Equation 1:</u>  C(s)+2H_2O(g)\rightleftharpoons CO_2(g)+2H_2(g);K_{p1}

<u>Equation 2:</u>  H_2(g)+CO_2(g)\rightleftharpoons H_2O(g)+CO(g);K_{p_2}

The net equation follows:

C(s)+CO_2(g)\rightleftharpoons 2CO(g);K_{p}

As, the net reaction is the result of the addition of first equation and the twice of second equation. So, the equilibrium constant for the net reaction will be the multiplication of first equilibrium constant and the square of second equilibrium constant.

The value of equilibrium constant for net reaction is:

K_p=K_{p1}\times (K_{p2})^2

We are given:

K_{p1}=3.09

K_{p2}=0.793

Putting values in above equation, we get:

K_p=3.09\times (0.793)^2=1.94

Hence, the value of K_p for the net reaction is 1.94

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Answer:

64J of energy must have been released.

Explanation:

Step 1: Data given

One reactant contains 346 J of chemical energy, the other reactant contains 153 J of chemical energy.

The product contains 435 J of chemical energy.

Step 2:

Since the energy is conserved

Sum of energy of Reactants = Energy of Products

Sum of energy of Reactants = 346 J + 153 J = 499 J

The energy of the product = 435 J

435 < 499

This means energy must have been lost as heat.

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Coefficient of \rm C_2H_2 in this equation: 2.

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In other words, for every two moles of \rm C_2H_2 that this reaction consumes, two moles of \rm H_2O would be produced.

Equivalently, for every mole of \rm C_2H_2 that this reaction consumes, one mole of \rm H_2O would be produced.

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