The reaction is exothermic.
From H and O, oxygen is the most electronegative, so that the negative side of the H-O-H 'triangle' with O in top.
becoz pH is the negative log of H ions. pH=-log(H+)
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
It can be said to be exothermic since H is negative. Also below a temp of 3708ºC, the reaction will be spontaneous because ∆G will be negative. This is from ∆G = ∆H - T∆S.
G is always negative when H is negative and S is positive.
No, when H and S are both negative, the reaction will only be spontaneous below a certain temperature
You cannot simplify them. If they are negative they have to stay negative.
d/dh(h^-1) = -1(h^-2) = -(h^-2)
yes
1/h-8 = (1/h)-8 = h8
h
The reaction is exothermic.
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
From H and O, oxygen is the most electronegative, so that the negative side of the H-O-H 'triangle' with O in top.
becoz pH is the negative log of H ions. pH=-log(H+)
-h/3 -4 = 13 -h -12 = 39 -h = 39+12 -h = 51 h = -51