given equilibrium concencentration and Kc, add CO2, add reactant, find concentration
The following equilibrium process at 686 deg. C. CO2(g) + H2(g) f/r CO(g) + H20 (g) The equilibrium concentration of the reacting species are [CO]=0.050 M, [H2]=0.045 M, [CO2]=0.086 M, and [H2O]=0.040 M. I calculate Kc for the reaction at 686 deg. C. = .52 If CO2 is added to increase concentration ot 0.55 mol/L, what will th ...continues
given total pressure and equilibrium constant, calculate euilibrium partial pressure
The heterogeneous equilibrium process C(s) + CO2(g) f/r 2 CO(g) At 700 deg. C. the total pressure in this system is 4.71 atem. The equilibrium constant is 1.52, calculate the euilibrium partial pressures of CO2 and CO. PCO2=? atm PCO=? atm
given equilibrium pressure, calculate Kp
When heated, ammonium carbonate decomposes as follows. NH4CO2NH2(s) f/r2NH3(g)+CO2(g) At a certain temp, the equilibrium pressure of the system is 0.318 atm. Calculate Kp for the reaction.
A quantity of 6.75 g of SO2Cl2 place in a 2.00 L flask. At 648 K, there is 0.0345 mol of SO2 present. Calc Kc for the reaction. SO2Cl2(g) f/r SO2(g)+Cl(g)
a mixture given moles of both, after reaction mole left, calculate Kc
A mixture containing 3.9 moles of NO and 0.88 mole of CO2 was allowed to react in a flask at a certain temp according to the equation NO(g)+CO2(g) f/r NO2(g)=CO(g) At equilibrium, 0.11 mole of CO2 present. Calc. equil. constant Kc.
calculate Kp given total pressure
NH4Cl(s) f/r NH3(g)+HCl(g) Calculate equilibrium constant Kp if the total pressure is 2.9 atm at this temp.
This topic teaches students basic principles required to solve problems involving PH calculation of srong acid and strong alkali. It also cosiders why solution of some salts may have PH value > 7 or < 7, as well as making students to know why water and ammonia are bases.
given product moles, volume, % reacted, find Kc
The following reaction occurs at 1600 deg. C. Br2(g)<>2Br(g) When 1.05 moles of Br2 are put in a 0.980 L flask, 1.20 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.
given concentration, change a product concentration, what is concentrations
Equilibrium process at 686 deg. C. C02(g)+H2<>CO(g)+H20(g) [CO2] is 0.086 M [H2] is 0.045 M [CO] is 0.050 M [H20] is 0.040 M Calculate Kc for the reaction at 686 deg. C. Which I did 0.050*0.040/.086*.045 = approx. .52 If add CO2 to increase it concentration to 0.55 mol/L, what will the concentrations off all the gases ...continues
given Kc, calculate partial pressures
The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 x 10^-3 at 527 deg. C. COCl2(g)<>CO(g)+Cl2(g) Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm Answer should give partial pressures of COCl2, CO, Cl2 I do not understand also what is meant b ...continues
