Janavi

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g) + O2(g) --> 2NO2(g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for this reaction at 298 K when t...

Consider the following reaction. A(aq) (Two way arrows) 2B(aq) Kc = 7.94*10^-6 at 500K If a 2.70 M sample of A is heated to 500K what is the concentration of B at equilibrium?

Calculate the change in pH when 5.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). (I have several problems like this can some one work this through for me as a base line)?

Delta G = G not + RTlnQ ==69.0 +(0.008314*298K*(ln((0.8^2)/((0.25^2)*0.15)) =-69.0 +10.46383111 =-58.53616889

How do I calculae the K for Reaction 2?

Some one please help I really do not understand this question one bit.

347

I did not calculate it for rxn 1 please please give me a step by step run down I honestly do not know how to do this problem and I have several more like it I really need a template to work off of to do the others please help me.

I can learn by example, this is an example please, work it out so I can do the rest. This question does not even count towards my final grade but the others like it do, so please help me.

Thank you Karan!

1: Set all the delta g's for solids equal to 0 2:Find thr delta g for the gases. 3:Find the delta g for the second equation. 4:Add the delta g's for the 2 questions together. 5: Solve for the value of Q using the equation -Delta G not =RTLnQ

Thank you sooo much Karan!

Thanks Karan!!

Wait so, you are getting 0.65 from the total mL but shouldnt this be 65/1000 or 0.065?

Some one please help

I found the answer to a however i keep doing something wrong for b