uppose a solution is initially made that only contains A at a concentration of 0.240 M. If the chemical equation defining the reaction is A(aq) <----> B(aq) + C(aq) and given an equilibrium constant of 4.16×10-5 for the reaction determine the concentration of C after equilibrium has been reached.
uppose a solution is initially made that only contains A at a concentration of 0.240 M....
A solution initially contains 0.1 M of I2 and 0.1 M of I-. The following reaction occurs and the equilibrium concentration for I2 is 0.01 M. What is the Kc for the reaction? I2 (aq) + I- (aq) ---> I3- (aq)
We have a solution that has a concentration of 0.348 M for A(aq) and 0.619 M for B(aq). There are no other solutes initially. The reaction 2 A(aq) + B(aq) <---> 2 C(aq) + D(aq) takes place. At equilibrium, the concentration of C(aq) is 0.142 M. What is the equilibrium constant of this reaction? Please use at least 5 decimal places in calculations.
For the lonization of ammonia shown below, the mixture initially contains 0.500 M NH, (aq). Determine the equilibrium millimolar (mm) concentration of HO- if K. - 1.74 x 10-5. NH3 (aq) + H2O (liq) + NH4+ (aq) + OH- (aq) QUESTION 18 Calculate the concentration of sulfate (SO2-) in a 0.0500 M solution of Nasso, If K = 0.012 for the following reaction: HSO4- (aq) + H20 (lia) = H2O* (aq) + SO42- (aq)
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.35 M , and [C] = 0.700 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.240 M and [C] = 0.860 M . Calculate the value of the equilibrium constant, Kc. Express your answer numerically.
Sodium phosphate is added to a solution that contains 0.0094 M aluminum nitrate and 0.025 M calcium chloride. The concentration of the first ion to precipitate (either Al^3+ or Ca^2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate? Sulfur dioxide reacts with chlorine at 227 degree C: SO_2(g) +Cl_2(g) SO_2Cl_2(g) K_p for this reaction is 5.1 times 10^-2 atm-1. Initially, 1.00 g each of SO_2 and Cl_2 are placed...
The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=2.0 Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express the molar concentration numerically using two significant figures. Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express the molar concentration numerically using two significant figures.
Part A)The reversible chemical reaction . A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=2.6 Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Part B) What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express your answer to two significant figures and include the appropriate units.
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3 and 0.200 M KCN. The formation constant for [Ag(CN)2] (aq) is Ka= 1.0 x 10^21. Show your work for each step. a. 5.6 x 10^-22 M b. 5.0 X 10^-22 M c. 3.3 x 10^-33 M d. 1.0 x 10^-30 M e. 1.3 x 10^-21 M
Question We have a solution that has a concentration of 0.340 M for Alaq) and 0.599 M for B(aq). There are no other solutes initially. The reaction 2 A(aq) + (aq) --> 2 Claq) + (aq) takes place. At equilibrium, the concentration of Claq) is 0.160 M. What is the equilibrium constant of this reaction? For the reaction 2 Alaq) + Cla), the standard Gibbs free enthalpy change is 141 kJ at 25°C. The initial concentration of Alaq) is 0.540...
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C? Express your answer using two significant figures.