# Chemistry

posted by .

One mole of N2 and three moles of H2 are placed in a flask at 375 C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31*10^4.

I assume this to be the reaction
N2 + 3H2 --> 2NH3

Help ?

Forgot to mention: Final answer is 50 atm

• Chemistry -

...............N2 + 3H2 ==> 2NH3
begin (mols)..1.0...3.0......0
change.........-x.....-3x.....2x
final........1.0-x..3-3x.....2x

total n = 1.0-x+3-3x+2x = 4-2x
And we know mol fraction NH3 = 0.21; therefore,
(2x)/(4-2x) = 0.21 and solve for x = moles.
Use x to determine moles NH3, moles H2 and moles N2 at equilibrium.
Then determine mole fraction N2, NH3(which you have) and H2.
PNH3 = 0.21*Ptotal
PH2 = XH2*Ptotal
PN2 = XN2*Ptotal
Then substitute partial pressures into Kp expression and solve for P. By the way, I think Kp is too large; in fact, I suspect it should be 10^-4 and not 10^4; i.e., I think you made a typo.

## Similar Questions

1. ### AP CHEM!

IM SO CONFUSED PLEASE HELP! H2 +CO2-->H2O + CO When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured. [H2]= 0.20mol/L …
2. ### chemistry

For the following reaction: 2NH3 ----> N2 + 3H3 6.42 moles of NH3 were placed in a 7.4 L flask and allowed to come to equilibrium. 3.60 moles of NH3 remain at equilibrium. Calculate Kc for the reaction.
3. ### chemistry

For the following reaction: 2NH3 ----> N2 + 3H3 6.42 moles of NH3 were placed in a 7.4 L flask and allowed to come to equilibrium. 3.60 moles of NH3 remain at equilibrium. Calculate Kc for the reaction.
4. ### Chemistry

At a particular temperature, k=1.6x10^-5 for the reaction 2SO3(g)=2SO2(g)+ O2 If 4 mole of SO2 and 2 mole of O2 are placed into a 2.0 L flask, calculate the equilibrium concentration of all the species. Thanks.
5. ### Chemistry

One mole of N2 and three moles of H2 are placed in a flask at 375 C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31*10^4. I assume this to be the reaction …
6. ### Chemistry

Which pair of samples contains the same number of hydrogen atoms two moles of NH3 and three moles of N2H4 two moles of NH3 and one mole of N2H4 four moles of NH3 and three moles of N2H4 one mole of NH3 and one mole of N2H4
7. ### chemistry

Ammonium bisulfide, NH2HS, forms ammonia NH3, and hydrogen sulfide, H2S through the reaction: NH4HS (s) <--> NH3(g) + H2S(g) Kp value of .120 at 25C in a 5L flask is charged with .300g of H2S at 25C. A) What are the partial pressures …
8. ### science-chemistry

please anwser soon, a rigid 4.10L flask contains a mixture of 1.25 moles of H2, 0.250 mole of O2, and sufficient Ar so that the partial pressure of Ar in the flask is 1.00 atm. The temperature is 63.5 degrees C A) Calculate the total …
9. ### Chemistry

At 400°C the reaction H2+I2<->2HI has an equilibrium constant Kp value of 55.5. A mixture of 1 mole of H2 and 1 mole of I2 is placed in a flask and heated to 400°C. Calculate the mole fraction of HI in the mixture of gases …
10. ### Chemistry

One mole of N2 and 3 moles of H2 are placed in a flask at 375 degree celsius.?

More Similar Questions