1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a 4.00 L container. CH4(g)+2H2O(g)????CO2(g)+4H2(g) At equilibrium, 4.89 g CO2 is present. Calculate Kc.
2. At a certain temperature, 0.352 mol CH4 and 0.862 mol H2S are placed in a 1.50 L container. CH4(g)+2H2S(g)????CS2(g)+4H2(g) At equilibrium, 14.5 g CS2 is present. Calculate Kc .
3. At a certain temperature, 0.3211 mol of N2 and 1.501 mol of H2 are placed in a 2.50 L container. N2(g)+3H2(g)????2NH3(g) At equilibrium, 0.1001 mol of N2 is present. Calculate the equilibrium constant, Kc.
4. Phosphorus pentachloride decomposes according to the chemical equation PCl5(g)????PCl3(g)+Cl2(g)Kc=1.80 at 250° C A 0.172 mol sample of PCl5(g) is injected into an empty 2.65 L reaction vessel held at 250° C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a...
At a certain temperature, 0.338 mol CH4 and 0.831 mol H2O is placed in a 3.50 L container.CH4(g)+2H2O(g)↽−−⇀CO2(g)+4H2(g)At equilibrium, 6.51 g CO2is present.Calculate ?c. _______
At a certain temperature, 0.361 mol CH4 and 0.972 mol H2S are placed in a 4.00 L container. CH4(g)+2H2S(g)↽−−⇀CS2(g)+4H2(g) At equilibrium,11.3 g CS2 is present. Calculate ?c The answer is NOT 1.17e2, 9.57e-6, or 6.8e-5, Please show me how you got your answer. Thank you.
At a certain temperature, 0.4811 mol of N2 and 1.801 mol of H2 are placed in a 2.50 L container. N2(g)+3H2(g)−⇀↽−2NH3(g) At equilibrium, 0.1001 mol of N2 is present. Calculate the equilibrium constant, Kc. Kc=
Please help.. . At a certain temperature, 0.3811 mol of N2 and 1.641 mol of H, placed in a 2.50 L container are N2 (g)3 H2 (g)= 2 NH3 (g) At equilibrium, 0.1001 mol of N, is present. Calculate the equilibrium constant, Kg. Kc
At a certain temperature, 0.3211 of N2N2 and 1.701 mol of H2H2 are placed in a 2.00 L container. N2(g)+3H2(g)↽−−⇀2NH3(g) At equilibrium, 0.1801 mol of N2N2 is present. Calculate the equilibrium constant, ?c
At a certain temperature, 0.4411 mol of N2 and 1.581 mol of H2 are placed in a 1.50 L container.N2(g)+3H2(g)⇌2NH3(g)At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.Kc=_____
At a certain temperature, 0.4411 mol of N2 and 1.521 mol of H2 are placed in a 3.00 L container. N2(g)+3H2(g)−⇀↽−2NH3(g) At equilibrium, 0.1601 mol of N2 is present. Calculate the equilibrium constant, Kc.
At a certain temperature, 0.4011 mol of N, and 1.541 mol of H, are placed in a 2.00 L container. N2(g) + 3H2(g) = 2 NH3(g) At equilibrium, 0.1201 mol of N, is present. Calculate the equilibrium constant, Kc. Kc =
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
on 27 of 37 > At a certain temperature, 0.900 mol So, is placed in a 4.00 L container. 2 503(g) = 2 802(g) + O2(g) At equilibrium, 0.110 mol O, is present. Calculate Kc. Kc =