At equilibrium, the concentrations in this system were found to be [N₂] = [0₂] = 0.200 M and [NO] = 0.500 M. N₂(g) + O₂(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NO] final 0.202 Incorrect M At a certain temperature, the Kp for the decomposition of H₂S is 0.704. H₂S(g) = H₂(g) + S(g) Initially, only H₂S is present at a pressure of 0.260 atm in a closed container. What is the total pressure in the container at equilibrium? Ptotal = atm

The initial concentrations of Na+ and C1 in the reaction below are each 0.0434 M. If the initial concentration of NaCl is 0 M and the equilibrium constant is Kc = 8.21 under certain conditions, what is the equilibrium concentration of Nat? NaCl(aq) = Na+ (aq) + Cl¯ (aq) Select the correct answer below: 0.0287 M 0.0354 M 0.0432 M -4 6.81 x 10 M

2C2H2(g) + 5O2(g)  4CO2(g) + 2H2O(g) You have 0.4 moles C2H2 and 0.2 moles O2 present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process?   Question 5 options:   Conc. C2H4 O2 CO2  H2O   Initial 0.4  0.2  0  0   Change  -x -x  +x  +x   Equil.  0.4-x 0.2-x  x  x    Conc. C2H4 O2 CO2  H2O   Initial 0.08  0.04 0  0   Change  -2x -5x  +4x  +2x   Equil.  0.08-2x 0.04-5x  4x  2x    Conc. C2H4 O2 CO2  H2O   Initial 0.4  0.2  0  0   Change  -2x -5x  +4x  +2x   Equil.  0.4-2x 0.2-5x  4x  2x    Conc. C2H4 O2 CO2  H2O   Initial 0.08 0.04 0  0   Change  -20x -20x  +20x  +20x   Equil.  0.08-20x 0.04-20x  20x  20x

You are an industrial chemist working for a company that makes methanol (CH3OH) according to the equilibrium reaction shown below.  You love your job, except that your assistant does not have the best notebook keeping skills.  One day you set up the reaction with the equilibrium concentrations shown below.    CO (g)   +   2 H2 (g)    <-->  CH3OH (g) 0.24 M        1.1 M                  0.15 M        at 327oC Later on your assistant mentions that he added some more CO, but he doesn't remember how much.  But he also remembers that as the equilibrium was being reestablished, the hydrogen concentration changed by 0.3 M, although he doesn't remember if it went up by that much, or down by that much.  How much carbon monoxide did he add, in M?

At a certain temperature, the K₂ for the decomposition of H₂S is 0.704. H₂S(g) = H₂(g) + S(g) Initially, only H₂S is present at a pressure of 0.260 atm in a closed container. What is the total pressure in the container at equilibrium? Ptotal = atm

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Use equilibrium concentrations to calculate K.   Some NOBr is placed in a flask and heated to 475 K. When equilibrium is reached, the flask is found to contain NOBr (2.14×10-2 M), NO(2.66×10-2 M), and Br2 (2.98×10-2 M). What is the value of the equilibrium constant for the following at reaction at 475 K?2NOBr(g)-------> 2NO(g) + Br2(g)         K =

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