4 mL of 5 x 10-3 M Fe(NO3)3 is added to 6 mL of 8x10-3 MKSCN along with 4 mL of water. The concentration of FeSCN2+ was found to be 3 x 10-4 at equililibrium. How many initial moles of Fe3+ are present in the solution? How many initial moles of SCN-are present in the solution?  How many initial moles of FeSCN2+ are present

The equilibrium constant for H2O(g)      +    CO(g)     ↔      H2(g)   +    CO2(g)   is 1.30 at 730  0C. At the start of the reaction there are 0.05 mol of H2O (g) and 0.0600mol CO (g) in a 4.00-liter reaction chamber. What are the concentrations of all the gases when equilibrium is established?

A student ran the following reaction in the laboratory at 744 K:N2(g) + 3H2(g)      2NH3(g)When she introduced 4.00×10-2 moles of N2(g) and 5.96×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.88×10-4 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

Consider the following equilibrium reaction:CO + H2O ⇌ CO2 + H2; Kc = 1.56If 1.00mol of CO is mixed with 3.00mol of H2O in a 1.00L container, what is the concentration of H2 atequilibrium?

A student ran the following reaction in the laboratory at 695 K:N2(g) + 3H2(g)      2NH3(g)When she introduced 4.09×10-2 moles of N2(g) and 7.14×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 1.99×10-3 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

Choose the equilibrium constant expressions for the following reactions. a) 2SO2(g) + O2(g)  2SO3(g)      Keq =   b) CS2(g) + 4H2(g)   CH4(g) + 2H2S(g)                            Keq =

3. Ca(OH)2(s)⇄Ca2+(aq)+2OH−(aq)Ksp=5.5×10−6 at 298KThe equilibrium in a saturated solution of Ca(OH)2 is represented above. In an experiment, a student places 5.0 g of Ca(OH)2(s) into 100.0 mL of distilled water and stirs the mixture. How would the results be affected if the student repeats the experiment but this time places 5.0 g of Ca(OH)2(s) into 100.0 mL of 0.0010 M NaOH(aq) instead of distilled water?a)Less solid will dissolve, because the larger value of [OH−] will cause the equilibrium position to lie farther to the right.b)Less solid will dissolve, because the larger value of [OH−] will cause the equilibrium position to lie farther to the left.c)More solid will dissolve, because the larger value of [OH−] will cause the equilibrium position to lie farther to the right.d)More solid will dissolve, because the smaller value of [OH−] will cause the equilibrium position to lie farther to the left.

A student ran the following reaction in the laboratory at 1101 K:2SO2(g) + O2(g)      2SO3(g)When she introduced 0.104 moles of SO2(g) and 0.101 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 7.28×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

The equilibrium constant, Ko, for the following reaction is 1.29x10-2 at 600K. cocl,(g) co(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.265 moles of COCI,(g) are introduced into a 1.00 L vessel at 600K. [CoCl,] = M [CO] M [Cl,] M

In an experiment where the initial concentration of Fe3+ was 0.00171 M and the initial concentration of SCN- was 0.000434 M, a student measured the final equilibrium concentration of FeNCS2+ to be 0.000182 M. Fe3+(aq) + SCN-(aq) ↔ FeNCS2+(aq) Calculate the final equilibrium concentration of Fe3+