Thank you for registering.

One of our academic counsellors will contact you within 1 working day.

Please check your email for login details.
MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping

If ΔG° a reaction is positive, then the reaction will not proceed at all, in the forward direction for any concentration of the reactants and the products. This statement is false. Explain.

If ΔG° a reaction is positive, then the reaction will not proceed at all, in the forward direction for any concentration of the reactants and the products. This statement is false. Explain.

Grade:upto college level

1 Answers

Sunil Kumar FP
askIITians Faculty 183 Points
7 years ago
yes the statemenrt is not true .
we know that ×G =×H - T×S
where ×represents delta
delta h -ve ,delta s +ve always spontaneous
h=+ve s=-ve non spontNeous at lll temperature
h=+ve s=+ve spontaneous at high temperatue
h=-ve s=-ve zpontaneous at low temperarure
in the reaction of the formation of NO and No2 the standard free energy change is 87.6kj/mole and 51.3kj/mole .yet we see the formation of NO and NO2.
N2 + O2----2NO
NO + .5 O2------NO2

thus we see that although delta g is positive yet the reaction occurs

thanks and regards
sunil kumar
askIItian faculty

Think You Can Provide A Better Answer ?

Provide a better Answer & Earn Cool Goodies See our forum point policy

ASK QUESTION

Get your questions answered by the expert for free