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Ok I have a problems in a questions of Equilibria:
1. When calculating Kp, what are the total number of moles? The number of moles at equilibrium?
2. Finding moles at equilibrium from given data: CO2 + H2 <==> CO + H2O
A mixture containing 0.5 mol of Co2 and H2, with 0.2 moles of H2O and CO was placed in 1.0 dm^3 of container and was allowed to come to equilibrium at 1200k. KC at 1200k is 1.44,
Calculate the moles at equilibrium of each of the substances at 1200k.
Answer: CO2 and H2 = 0.32, CO and H2o= 0.38
Please explain in full detail. Thanks!
3. N2O4 <===> 2NO2 1.0 mole of N2O4 was allowed to reach equilibrium at 400k. At equilibrium the partial pressure of N2O4 was found to be 0.15 atm,
Givent that Kp for this equilibrium is 48 atm, calculate the partial pressure for No2 in the equilibrium mixture.
Answer: 2.68 atm
Please explain in full detail and show all the working.you would help a ton. thanks in advance!
1. When calculating Kp, what are the total number of moles? The number of moles at equilibrium?
2. Finding moles at equilibrium from given data: CO2 + H2 <==> CO + H2O
A mixture containing 0.5 mol of Co2 and H2, with 0.2 moles of H2O and CO was placed in 1.0 dm^3 of container and was allowed to come to equilibrium at 1200k. KC at 1200k is 1.44,
Calculate the moles at equilibrium of each of the substances at 1200k.
Answer: CO2 and H2 = 0.32, CO and H2o= 0.38
Please explain in full detail. Thanks!
3. N2O4 <===> 2NO2 1.0 mole of N2O4 was allowed to reach equilibrium at 400k. At equilibrium the partial pressure of N2O4 was found to be 0.15 atm,
Givent that Kp for this equilibrium is 48 atm, calculate the partial pressure for No2 in the equilibrium mixture.
Answer: 2.68 atm
Please explain in full detail and show all the working.you would help a ton. thanks in advance!