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☆☆☆☆☆HCI (Hydrochloric acid)
increased temperture causes rate or reaction to increase.
For a reaction whose slowest step is
mX + nY ----> aXY
rate = k * [X]m * [Y]n
where k is the rate constant; brackets represent concentrations; m and n are exponents on the concentrations of X and Y, respectively
The rate of the reaction begins to decrease as reactants are used up
Rate = k[A]m[B]n
Strong Intermolecular Forces attract the molecules
I suspect it could be " k eq 1" , or "k =1".
Increasing temperature affects a reaction in two ways:
1) at higher temperatures the molecules are moving around faster and collisions and reactions are more frequent, so the reaction - both forward and reverse - speed up.
2) at higher temperatures, the equilibrium state will shift. In some cases it will shift the equilibrium towards the product. In other cases, it will shift it back towards the reactants.
the rate would be four times larger. apex
Ka= 1.62 x 10-12
Ka = [H+][CN-]
---------------
[HCN]
increasing the concentration in the molecue
The pH is 5,6.
Reactants are favored over products in the reaction.
