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3 years ago

Balance the following reaction in acidic solution:. . Ag(s) + NO3-(aq) -> Ag+(aq) + NO(g)

1 answer:

3 0

The two half-reactions are...
Ag→Ag+
and...
NO3→NO
Let's start by balancing the first half-reaction...
Ag→Ag+
The amounts are already balanced; 1:1. The oxygens are balanced. So all that's left is to balance the charge...
Ag→Ag++e−
Now let's do the other equation... Amounts of nitrogen are balanced, so we first need to balance the oxygens...
NO3→NO
4H++NO3→NO+2H2O
Next, we need to balance charge...
4e−+4H++NO3→NO+2H2O
Now let's go ahead and rewrite each half-reaction after being balanced by themselves...
Ag→Ag++e−
4e−+4H++NO3→NO+2H2O
Now we need to multiply by some factor to get the electrons to cancel out. In this case, that factor is 4, which needs to be applied to the top half-reaction...
4(Ag→Ag++e−)=4Ag→4Ag++4e−
Then we combine this half-reaction with the second one above to get...
4Ag+4H++NO3→4Ag++NO+2H2O

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All of these are true

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Which of these molecules and polyatomic ions cannot be adequately described using a single Lewis structure? Check all that apply

11Alexandr11 [23.1K]

<h3><u>Answer;</u></h3>

CO3^2- and O3

<h3><u>Explanation;</u></h3>

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3 years ago

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 $K_1 \& K_2$ :

$K=K_1\time (K_2)^2$

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3 years ago

What is the chemical formula for iron(II) hydroxide?

makkiz [27]

Answer: Fe(OH)2

Explanation: Fe has a charge of 2+ and OH has a charge of 1-. Switch the charges of the two elements to get the formula of Fe(OH)2.

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2 years ago

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ziro4ka [17]

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