Question

10.0 moles of NH3 and 10.0 moles of H2 are introduced into a 1.00 L flask. At equilibrium, 3.0 moles of NH3 gas remain. Calculate Kc for this reaction.

N2(g) + 3H2(g) < > 2NH3(g)

sorry i forgot to say show all the work please!

We usually don't do the whole problem. The idea on this board is to help you do your own homework, not to do it for you. Here are some hints.
You have the equation. Write the Kc expression. From the knowledge that 3.0 mols NH3 gas remains at equilibrium, that must mean that 7 mol NH3 must have been used. Use that to determine equilibrium concentrations for N2 and H2, and plug into Kc equation. If this hint is not enough, please post your work and tell us exactly what you don't understand about it.

Five (5.00) grams of glucose, C6H12)6, is dissolved in 500.0 grams of acetic acid. What is the new freezing point and boiling point for the solution?
Kf acetic acid = 3.90, Kb acetic acid = 3.07
(normal freezing point for acetic acid = 16.60 dg C, boiling point = 118.5 dg C)

f.p. = ??????
b.p. = ??????