Calculate equilibrium constant Kc
Process at 700 deg. C. Reaction 2H2(g)+S2(g)>2H2S(g) < H2=2.5 moles S2=1.35 x 10^-5 mole H2S=8.70 mol Reacts in a 12.0 L flask. What is equilibrium constant Kc?
Calculate Kc when given moles and percent reacted
Reaction at 1600 deg. C Br2(g)>2Br(g) Br2=1.05 moles Br2 placed in .980 L flask 1.2% Br2 undergoes dissociation. Calculate equilibrium constant Kc for the reaction
Calculate Kp and Kc given percent reacted and total pressure
2NOBr(g)>2NO(g) + Br (g) Nitrosyl bromide, NOBr, is 34 percent dissociated at 25 deg. C and the total pressure is 0.25 atm. Calculate kp and kc for the dissociation.
Calculate Kp and Kc given percent reacted and total pressure
2NOBr(g)>2NO(g) + Br (g) Nitrosyl bromide, NOBr, is 34 percent dissociated at 25 deg. C and the total pressure is 0.25 atm. Calculate kp and kc for the dissociation.
2 equilibrium constants(Kp'and Kp") find Kp
This is problem having troubles with. Determined at 1123 K. C(s)+Co2(g) >2CO(g) K'p=1.3 x 10^14 < CO(g) + Cl2(g)>COCl2(g) K"p=6.0 x 10^-3 Equilibrium constat expression Kp for reaction C(s) + CO2(g)+2Cl2(g)>2COCl2(g) Kp=(PCOCL2)^2/((PCl2)^2 x (PCO2)) Calculate the equilibrium constant at 1123K ...continues
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.
