Search found 6 matches

Sat Jan 11, 2020 11:24 am
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Q and relation of [R] to [P]
Replies: 5
Views: 91

Re: Q and relation of [R] to [P]

K is the fixed ration of the concentrations of the products to the reactants. If the Q, which means the ratio of the concentrations of products to reactants, is smaller than the K, than that means there aren't enough products in this reaction to be at equilibrium. So the concentrations of the produc...
Sat Jan 11, 2020 11:19 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Knowing it's an Equilibrium Reaction
Replies: 4
Views: 45

Re: Knowing it's an Equilibrium Reaction

I think in this class we will be given the double arrow, as it is an easy way to understand if the reaction is reversible or not.
Sat Jan 11, 2020 11:14 am
Forum: Ideal Gases
Topic: pressure [ENDORSED]
Replies: 13
Views: 365

Re: pressure[ENDORSED]

PV=nRT so if you increase the temperature and the number of moles and keep the volume constant, you can increase pressure.
Sat Jan 11, 2020 11:12 am
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Q
Replies: 10
Views: 106

Re: Q

Q is not a fixed ratio like K is. Which means that Q is the ratio of the concentrations and the partial pressures of the products to those of the reactants at that moment in the reaction.It is essentially K but doesn't have to be equal to K. So yes, I think it can be applied to both.
Sat Jan 11, 2020 11:07 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: K vs. Q
Replies: 10
Views: 108

Re: K vs. Q

K and Q have the same values at equilibrium. That is why, if they are not equal you can see whether the reaction going forwards or backward by comparing the Q and the K. If Q is bigger than K, that means the reaction at this time has more products than it's equilibrium state, which is what the K val...
Sat Jan 11, 2020 11:01 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Change in k
Replies: 11
Views: 191

Re: Change in k

According to Le Chatelier's Principle, an equilibrium will act to minimize external disturbances. So, if you increase the concentration of (let's say) the product, the equailibriım will start relying more on to the left side to produce more reactants. This will diminish the change done to the system...