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A system that is not at equilibrium is found to contain 0.250 M of A (aq), 0.250 M of B(aq), and 0.290 M of C (aq). Note that each of these species are hypothetical and do not represent actual elements from the periodic table. The reaction involving these three species is shown below. A (aq) +B(aq) (aq) K = 0.670 a) What is the value of Q. for the system based on the conditions described above? Q: b) Which direction would the reaction proceed in order to reach equilibrium? Shift left to form more reactants Shift right to form more products The system is already at equilibrium c) Determine the concentration of each of the three species once the system reaches equilibrium A: M B M C M
Hydrazoic acid HN,, has a K, value of 1.9 X 10 If you prepare a 0.240 M solution of HIN,, answer each of the questions listed below a) Based on the information provided above, fill in the ICE table below inputting x for any relative changes. Be sure to indicate the direction of change, ie. +/- Be sure to use the proper number of significant figures. Any zeroes should be denoted as 0. The equilibrium row should contain the x variable HN: (aq) + H.0 (1) ལྟ་ Ns (aq) H:0+ (aq 1 E b) Determine H.O once the reaction reaches equilibrium HO: M c) Determine the pH of the system when it reaches equilibrium pH:
Assume that 0.520 M of A (g) and 1.40 M of B (g) are sealed in a reaction vessel and undergo the reaction shown below A(g) + 3B (g) = 2(8) a) Based on the information provided above ONLY, fill in the ICE table below inputting x for any relative changes. Be sure to indicate the direction of change le +/- Be sure to use the proper number of significant figures. Any zeroes should be denoted as 0. The equilibrium row should still contain the x variable. A (g) 3B 20(%) c E b) Determine the value of *, if there is 0.110 M of A (g) remaining once the reaction reachet equilibrium M c) Based on parts and bl, determine the value of the equilibrium constant for the reaction K: