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I need help with Chemical Equilibrium for Chemistry1?
1. For the reaction: 2NO(g) + H2(g) --->N2O(g) + H2O(g) + energy
2. Write the equilibrium constant expression for the reaction.
3. What effect would an increase in temperature have on the reaction rate?
4. Assume the reaction is a single-step reaction. What would be the effect on the reaction rate if the [H2] were doubled?
5. Assume the reaction is a single-step reaction. What would be the effect on the reaction rate if the pressure on the reaction were doubled?
6. Assume the reaction is reversible and at equilibrium. What shifts in the equilibrium of this reaction are suggested by Le Chatelier's Principle?
1- The energy produced as a product indicates that this is an exothermic reaction.
2- Equilibrium constant expression is the concentration of the products multiplied together divided by the concentration of the reactants multiplied together
for all compounds in the expression concentration is denoted by square brackets around the compound, and they are all to the power of their ratio (the number before the chemical compound i.e. it would be [NO]^2
3- As it is an exothermic reaction, and according to Le Chatelier's principle, any equilibrium will try and oppose a change, and an increase in temperature would favour the reverse reaction as it would be endothermic and therefore oppose the increased heat.
4- It would increase as long as chances of collisions would increase.
5- It would increase the rate of reaction as the chance of a collision between particles with the required activation energy would be greater.
6:
4- As there is no number in front of the H2 it's order is 1. That means that what happens to that, happens to the rate of reaction. (But if this was with respect to the NO2 what happens to it would do the same to the rate of reaction but squared as it has a 2 in front of it, therefore making the order of reaction with respect to it 2. e.g. is NO2 was doubled, rate would quadruple.)
5- As they are all gasses, and there are more moles of gas on the left, you can apply Le Chatelier's principle once again. Increase in pressure will make the equilibrium want to decrease the pressure-the way to do this is to make less moles of gas as one mole of gas occupies the same volume no matter what it is. Therefore it would favour the forward reaction.
I know its a little long winded-but I hope it helps 
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