LSGH General Chemistry 2 Final Exam

Calculate the mass of KI in grams required to prepare 500 mL of a 2.80 M

solution (MW of KI = 166.0028 g/mol).

How many moles of MgCl2 are present in 60.0 mL of 0.100 M MgCl2 solution (MW of MgCl2 = 95.211 g/mol)?

Calculate the molarity of each of 29.0 g of ethanol (C2H5OH) in 545 mL of solution (MW of ethanol = 46.068 g/mol).

Calculate the volume in milliliters of a solution required to provide 2.14 g of sodium chloride (NaCl) from a 0.270 M solution (MW of NaCl = 58.44 g/mol).

Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate, Ba(OH)2 · 8H2O. What mass of Ba(OH)2 · 8H2O would be required to make 500.0 mL of a solution that is 0.1500 M in hydroxide ions (MW of barium hydroxide = 171.34 g/mol)?

Write the reaction rate expressions for the following reactions in terms of the disappearance of the reactants and the appearance of products:

Consider the reaction in the figure. Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.066 M/s. (a) At what rate is NO2 being formed? (b) At what rate is molecular oxygen reacting?

The rate law for a reaction is given by rate = k[NH4+][NO2−]. At 25°C, the rate constant is 3.0 × 10−4/M · s. Calculate the rate of the reaction at this temperature if [NH4+] = 0.26 M and [NO2-] = 0.080 M.

Consider the reaction A + B ⟶ products. Using the data obtained at a certain temperature, as reflected in the figure, determine the order of the reaction and calculate the rate constant.

The following gas-phase reaction was studied at 290°C by observing the change in pressure as a function of time in a constant-volume vessel: ClCO2CCl3(g) ⟶ 2COCl2(g). Determine the order of the reaction and the rate constant based on the data in the figure, where P is the total pressure.