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Simora [160]
2 years ago
6

According to coulomb’s law, what happens to the potential energy of two oppositely charged particles as they get closer together

?.
Chemistry
2 answers:
ValentinkaMS [17]2 years ago
8 0

Answer:

According to coulomb's law their potential energy will increase and the particles will repel each other.

lesya [120]2 years ago
6 0
Answer :According to Coulomb's law, for opposite charges, the potential energy is [positive/negative] and becomes more [positive/negative] as the particles get closer together.
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How many neutrons does element X have if its atomic number is 56 and its mass number is 161?
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The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia: 2N0(g) +02(g) 2NO2 (g) The
Tresset [83]

The question is incomplete, complete question is :

The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia:

Step 1 : 4NH_3(g)+5O_2(g)\rightleftharpoons 4NO(g)+6H_2O(g)

Step 2 :  2NO(g) +O_2(g) \rightleftharpoons 2NO_2 (g)

The net reaction is:

4NH_3(g)+7O_2(g)\rightleftharpoons 4NO_2(g)+6H_2O(g)

Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K_1 and K_2. If you need to include any physical constants, be sure you use their standard symbols

Answer:

Equation that gives the overall equilibrium constant K in terms of the equilibrium constants K_1 \& K_2:

K=K_1\time (K_2)^2

Explanation:

Step 1 : 4NH_3(g)+5O_2(g)\rightleftharpoons 4NO(g)+6H_2O(g)

Expression of an equilibrium constant can be written as:

K_1=\frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^5}

Step 2 :  2NO(g) +O_2(g) \rightleftharpoons 2NO_2 (g)

Expression of an equilibrium constant can be written as:

K_2=\frac{[NO_2]^2}{[NO]^2[O_2]}

The net reaction is:

4NH_3(g)+7O_2(g)\rightleftharpoons 4NO_2(g)+6H_2O(g)

Expression of an equilibrium constant can be written as:

K=\frac{[NO_2]^4[H_2O]^6}{[NH_3]^4[O_2]^7}

Multiply and divide [NO]^4;

K=\frac{[NO_2]^4[H_2O]^6}{[NH_3]^4[O_2]^7}\times \frac{[NO]^4}{[NO]^4}

K=\frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^7}\times \frac{[NO_2]^4}{[NO]^4}

K=K_1\times \frac{[NO_2]^4}{[O_2]^2[NO]^4}

K=K_1\times (\frac{[NO_2]^2}{[O_2]^1[NO]^2})^2

K=K_1\time (K_2)^2

So , the equation that gives the overall equilibrium constant K in terms of the equilibrium constants K_1 \& K_2:

K=K_1\time (K_2)^2

4 0
3 years ago
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