A reaction, given below, is being followed spectroscopically to determine the concentrations of A, B, C and D. Based on the data shown, determine the value of the equilibrium constant. 2 A (aq) + B (aq) → 2 C (aq) + D (aq) Kc = ? Reaction [A], M [B], м [C], м [D], M time 30.0 0.500 0.450 minutes 60.0 0.460 0.480 0.040 0.020 minutes 120.0 0.420 0.460 0.080 0.040 minutes 240.0 0.420 0.460 0.080 0.040 minutes

For the general gas phase reaction A + 2 B ↔ 2 C + 2 D calculate the value of the equilibrium constant given the following equilibrium concentrations (report your answer to 3 significant figures in decimal format, not scientific notation): concentration of A = 2.78 Mconcentration of B = 2.88 Mconcentration of C = 0.103 Mconcentration of D = 0.193 M

Consider the following heterogenous reaction: 2AB(s) + C3(aq) + 4D(aq) ⇌ 2ABCD(aq) + CD2(l) The initial concentration of C3 is 0.20 M and 0.10 M for D. 5.0 g of reactant AB was also added. There were no products in the reaction flask at time 0. At equilibrium, the [D]eq = 0.03 M. (i) Will the concentration of reactant AB and product CD2 affect equilibrium? Explain why or why not. (i) Calculate the equilibrium constant, Kc for this reaction.

Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂(g) = 2 BrCl(g) Кр = 1.1 x 10-4 at 150 K A 209.0 L flask initially contains 0.901 kg of Br₂ and 1.104 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: 6.0 g

For the chemical equilibrium aA + bB 2 cC, the value of the equilibrlum constant Kis 25. What is the value of the equilibrium constant for the reaction cC aA+ bB? Type your answer. Submit

For the reaction 2 NH3 = 3H₂ + N₂ The equilibrium concentrations were found to be [NH3]=0.250 M [H2]=0.450 M [N2]=0.800 M. What is the equilibrium constant for this reaction?

Below is the concentration versus time graph for the reaction system. The graph was produced using secondary data at a temperature of 22 °C. 12.0- 10.0- 8.0- concentration (x10-2 M) 6.0 NO₂ 4.0+ 2.0+ 0.0 time (arbitrary units) i. Time t is shown on the graph above. Calculate the equilibrium constant at time f₁. ii. At time to the volume of the system was halved, keeping the temperature at 22 °C. Continue the graph to show how this change would affect the reaction system and how the system would respond to this change until equilibrium is restored. 4₁ 4₂

74x10+8 0.100 M, calculate the 104&the inale A + B 2C K = 1.0x103 If the observed concentrations at time t are all 0.100 M, will the reaction from that point on proceed to products or reactants? If the observed concentrations at time t are 0.400 M A, 0.500 M B and 0.0100 M C, will the reaction from that point on proceed to products or reactants? to enoiletineonoo muhdiliupe erlt etsluols M 00 s8 & A to O bns 8 A noitsineono lsitini edi 80xes.r=

Write the equilibrium constant expression for this reaction: 2 CH₂COO (aq)+C₂H6O₂(aq) → C6H1004(aq)+2 OH (aq) HEATIN RE 7² 3 7 FIN _ X S HOME P ? PO 10002 HEMER po HOTE ALUM KREMO M

For the reaction 2A ↔ B K = 13.686, if one started with 0.147 M A approximately how much A and B would be there be after equilibrium had been established?