00:01
The question, the following reaction is given, that is n2 plus o2, will give us two moles of no.
00:07
And in this table, the value of delta h -0, f, that is the enthalpyof formation, and s -not, that is, the entropy value is given.
00:15
And we need to calculate the delta -g -not value, that is, the standard reaction -free energy.
00:22
And for this, we'll be using the formula that is delta -g -0, this is equal to delta -h -0 -h -0 minus t delta s not so first we need to find out the delta h0 value so here we can write delta h0 this is equal to the summation of delta h0 f for the products minus the summation of delta h0 f for the products minus the summation of delta h0 f for the reactants so this is equal to so in the product side we have 2 moles of no.
01:06
So for no the value of delta h0 is 90 .3 and here we have 2 moles.
01:12
So that is why it will be 2 multiplied with 90 .3 and minus the delta h0f value for the reactants that is n to an 02, they are given as 0...