2. The equilibrium constant Kp for the reaction 2NO 2NO2 (g) = + O2 (g) (g) Is 158 at 1000 K. Calculate P 02 if P NO2 = 0.400 atm and P No = 0.270 atm. 3. Calculate the equilibrium constant (K.) for the following reaction: H2(9) + I2(g) = 2HI (g) where the equilibrium concentrations at 25.0 °C were found to be: [H2] 0.0505 M, [I2] = 0.0498 M, [HI] = 0.389 M %3D

Sagar chemistry

What is true about the forward and reverse reaction rates once chemical equilibrium is established?       The reverse rate is always faster than the forward rate.       Both the forward and reverse rates are equal       Impossible to determine because it depends on the reaction.       The forward rate is always faster than the reverse rate.

What happens to a system when products are added to a reaction vessel? O The amount of products increases. O The amount of reactants increases. O The amount of reactants decreases. O The system remains at equilibrium.

Question 29 of 30 Consider the reaction of N2O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190

I Review | Constants | Periodic Table Part B When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: The following system is at equilibrium:A(s) + 4B(g) = C(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help If a stress is applied to a reaction mixture at equilibrium,…

True/False. Explain your answer in one sentence or less.   In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.