You started with 0.60 M A and 0.80 M B Calculate equilibrium concentration of the element B.
A(aq) + 2B(aq) <--> 2C(aq)
Kc = 1.75 x 10^10
You started with 0.60 M A and 0.80 M B Calculate equilibrium concentration of the element...
Consider the reaction below. At equilibrium, the concentration of A is 7.000 M and the concentration of B is 8.000 M. If the equilibrium constant Kc = 0.2737, what is the equilibrium concentration of C? Pay attention to the phases of the substances before you proceed. Be sure to include units for a complete answer. Answer to 3 decimal places. 9A(s) + 8B(l) <-----> 2C(g)
Consider the reaction below. At equilibrium, the concentration of A is 0.0242 M and the concentration of B is 0.0767 M. If the equilibrium constant is Kc=0.0266, what is the equilibrium concentration of C? 3A(g)⇌3B(g)+2C(g) Round the answer to three significant figures.
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
For the following equilibrium: 3A+B↽−−⇀2C If equilibrium concentrations are [A]=1.1 M and [B]=1.4 M, and Kc=11.3, what is the equilibrium concentration of C? Your answer should have two significant figures.
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
For the following reaction, calculate the equilibrium concentration of CO (g). CO2 (g) + H2 (g) CO (g) + H20 (g) Kc = 0.11 [CO2] = 0.25 M [H2] = 0.80 M [H2O) = 0.50 M
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB (aq) To determine the equilibrium constant for this reaction at 298 K, a student mixes two solutions together and allows them to react: • 10.0 mL of 0.60 M A (aq), and, • 40.0 mL of 0.25 MB (aq). When this solution reaches equilibrium, the student measures the equilibrium concentration of AB in the 50.0 mL solution: [AB]E = 0.10 M. Which values should...
The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 2.3 M NO and 0.80 M Br2 , what is the molar concentration of NOBr? 2NOBr(g) = 2NO(g) + Br2 (g) Express your answer to two significant figures and include the appropriate units. Å R 0 2 ? [NOBr] = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
What are the concentrations at equilibrium of a 0.15 M solution of HCN? What will be the concentration of Cu2+(aq) at equilibrium? HCN(aq)<=>H+(aq) + CN–(aq) , Kc= 4.9 x 10-10
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What concentration of so-is in equilibrium with Ag,SO,(s) and 1.00 x 10-3 M Agt? The Kap of Ag,SO, can be found in this table. [s03-] = The Ksp of cadmium carbonate, CACO3, is 1.0 x 10-2. Calculate the molar solubility, S, of this compound. At 25 °C, only 0.0290 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25...