Question

An experiment was carried out to determine the value of the equilibrium constant Kc for the reaction.

Total moles of Ag+ present = 3.6 x 10-3 moles

Total moles of NH3 present = 6.9 x 10-3 moles

Measured concentration of Ag(NH3)2+ at equilibrium= 3.4* 10-2 M

Total solution volume = 100 mL

(a). Calculate the equilibrium concentration of Ag+ (uncomplexed).



(b). Calculate the equilibrium concentration of NH3 (uncomplexed).



(c). Calculate the value of the equilibrium constant (Kc).









I GOT 1.7*10^7 for question C. IS IT RIGHT?????????



What's the reaction? I'm guessing at
Ag^+ + 2NH3 ==> Ag(NH3)2^+
If that's the reaction my number is 1.75E7 which I would round to 1.8E7 instead of your 1.7E7. Good work.
THANX
uju
How

Related Questions

Initially, there are 33 moles of A and 0 moles of B. How many moles of A and B will be present after... Consider the following reaction: CO2 (g) + H2 (g) CO (g) + H2O (g) Calculate the value of the equil... For the reaction H2(g) + I2(g) <===> 2HI(g), Kc=54.9 at 699K. A system was charged with 2.50 moles o... Consider the following reaction CO2 (g) + H2 (g) ↔ CO (g) + H2O (g) Calculate the equilibrium co...