Answer Happy

At equilibrium: a. the total amount of reactants equals the total amount of products b. the concentration of each reactant equals the concentration of each product c. all chemical reactions have ceased d. the forward and reverse reactions are occurring at the same rate e. products are always favored

What is the pH of a 1 L solution containing 0.430 mol HC₂H3O2 and 0.190 mol NaC₂H302? K₂(HC₂H3O2) = 1.8 x 10-5. HINT: Begin by filling out the equilibrium table below. Balanced Equation HC₂H3O2 → H+ + C₂H30₂ Initial Concentration (M) Change (M) Equilibrium Concentration (M)

1. The equilibrium constant for the following reaction is 0.090: H2O(g) + Cl2O(g) 2 HQC(a) If 3.0 mol of H₂O gas and 3.0 mol of Cl20 gas are placed in a 2.00 L container and equilibrium is established. a) What is the equilibrium concentration of HOCI gas? Clearly show your steps? [4 marks] [2 marks] b) Calculate the percent reaction NOTE: percent reaction means percent yield. So this is a reflection of how much product you get vs how much you would have gotten if the reaction goes to 100% completion.

1. Calculate the pH of a 0.45 M solution of hydrazine (N2H4) [4]

1. Calculate the pH of a 0.048 M solution of NaCH3COO. (Sodium acetate) [4]

2. Given the equilibrium system N2(g) + 3 H2(g) 2 NH3(g) Kc = 0.065 at 450°C A 1.0 L reaction vessel is analyzed and found to contain 8.0 mol N2(g), 4.0x10² mol H2(g), and 4.4x10mol NH3(g). Is the system at equilibrium? If not predict the direction in which the reaction will proceed to reach equilibrium. [3 marks]