The decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas. 6 NO(aq) ⇌ 3 N 2 (aq) + 3 O 2 (aq) a) What is the equilibrium equation for the reaction above? b) What is the equilibrium expression for the reverse reaction.

Okay, guys. We're now going to look at practice question 1 that was left for us to do. So, for part a, it says, What is the equilibrium equation for the reaction above? Now, before you do any question like this, you should always check the phases of matter for your products and your reactants. They're all aqueous, so we're going to keep all of them. If any of them had been solids or liquids, we'd have to ignore them. Here we're going say k equals products over reactants anytime we're talking about the forward reaction. Here we're going to say it's going to be n2 cubed because its coefficient is 3 times O 2 cubed because again its coefficient is 3, divided by No6. So that would be our answer for the first one. Now, for part b, we're simply looking at the reverse reaction. So now K becomes reactants over products. So just switch everything. So now, No is on top, still to the 6 because the coefficient is 6 divided by n22 to the 3. It's as simple as that. Knowing this will help us solve the next practice question in which now we're given actual numbers and we're asked to find the equilibrium amount of No. Now, this is just doing the same exact thing we did before guys. Except now, I'm giving you what are k equals and I'm giving you some of the equilibrium concentrations of some of the compounds. Look to isolate the missing one. Here it's just basically using the algebra skills that we've developed and finding out what the concentration of No is. Good luck on it. If you get stuck, remember, click on the explanation button and watch a video of me explaining how I approach this same problem. Good luck.

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7. Energy, Rate and Equilibrium

The Equilibrium Constant

GOB Chemistry

7. Energy, Rate and Equilibrium

The Equilibrium Constant

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Multiple Choice

The decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas.
6 NO(aq) ⇌ 3 N₂(aq) + 3 O₂(aq)
a) What is the equilibrium equation for the reaction above?
b) What is the equilibrium expression for the reverse reaction.

Equilibrium expression for the forward and reverse reactions of nitrogen monoxide decomposition.

Equilibrium expression for the forward and reverse reactions of nitrogen monoxide decomposition with powers.

Equilibrium expression for the forward and reverse reactions of nitrogen monoxide decomposition with different powers.

Equilibrium expression for the forward and reverse reactions of nitrogen monoxide decomposition with cubic powers.

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Verified step by step guidance

Identify the balanced chemical equation for the decomposition of nitrogen monoxide: 6 NO(aq) ⇌ 3 N2(aq) + 3 O2(aq).

Understand that the equilibrium constant expression, K, is derived from the concentrations of the products and reactants at equilibrium.

For the forward reaction, the equilibrium expression is K = [N2]^3[O2]^3 / [NO]^6, where the exponents correspond to the coefficients in the balanced equation.

For the reverse reaction, the equilibrium expression is the reciprocal of the forward reaction's expression: K = [NO]^6 / [N2]^3[O2]^3.

Ensure that the equilibrium expressions are correctly set up with the concentrations raised to the power of their respective coefficients from the balanced equation.