[ashleighmarie08]

i'M HAViiNG TR0UBLE GETTiiNG STARTED WiiTH THESE PR0BLEMS (CAN S0ME0NE PLEASE SH0W ME THE STEPS 2 W0RK THEM...U D0N'T HAVE 2 ANSWER ALL 0F THEM...ANY HELP W0ULD BE APPRECiiATED!

1. What is the equilibrium concentration of CN1- ion in a solution prepared by mixing 60.0 mL of 0.160 M HCN and 60.0 ml of 0.160 M NH3?
NH3 + HCN ? CN1- + NH41+   K = 0.710

2. An equilibrium mixture contains 0.860 mol HI, 0.170 mol I2, and 0.200 mol H2 in a 1.00-L flask. What is the equilibrium constant for the following reaction?
2HI(g) ? H2(g) + I2(g)
How many moles of I2 must be removed in order to double the number of moles of H2 at equilibrium?

3. Consider the following equilibrium:
2NOBr(g) ? 2NO(g) + Br2(g)
An equilibrium mixture is 0.180 M NOBr, 0.312 M NO, and 0.162 M Br2.
a) What is the value of Kc at the temperature of the above concentrations?
b) How many moles/liter of NOBr must be added to the above equilibrium mixture to produce an equilibrium mixture that is 0.367 M Br2?
c) If the temperature is 390 K, what is the value of Kp?
d) What is the value of ?G? at 390 K?

4. At some temperature, K = 20.7 for the following reaction:
H2(g) + CO2(g) ? H2O(g) + CO(g)
The initial partial pressures of H2 and CO2 are each 3.00 atm.
What is the final pressure of CO?
What is the final total pressure?

[Borek]

Please read forum rules. Don't abuse capital letters.

In all cases the general approach is the same - you must write equation for equilibrium and equation (equations) for stoichiometry.

[Padfoot]

For Question 1 I suggest you use an ICE table
http://en.wikipedia.org/wiki/ICE_table