Suppose the following data are for the reaction: SO2Cl2 (g) → SO2 (g) + Cl2 (g) Time [SO2Cl2] 0 hr 0.618 M 4 0.500 10 .364 Calculate the value of the rate constant k if the reaction is first order in SO2Cl2 (g). (Suggestion: make a third column and use it to calculate the slope.) a. 0.030 hr-1 b. 0.053 hr-1 c. 0.023 hr-1 d. 0.125 hr-1 e. 0.036 hr-1 Tables.pdf Periodic Table with New Elements.pdf
Read DetailsSuppose a solution contains 0.7 M Ba2+ (aq) and 0.4 M Mg2+ (aq). Fluoride ions, F- , are then slowly added to the solution. Calculate the [Mg2+] left in solution when Ba2+ starts to precipitate, and then answer the following question. What percent of the original Mg2+ is left in solution when Ba2+ starts to precipitate? a. 3.5 x 10-5 % b. 6.8 x 10-2 % c. 6.8 x 10-4 % d. 3.5 x 10-7 % e. 2.7 x 10-2 % Tables.pdf Periodic Table with New Elements.pdf
Read DetailsSuppose you start with a solution that is at pH 8. If enough acid is added to make the [H+] 1000 times larger, what is the new pH? (Hint: Although this problem can be done using a calculator, it can easily be done in your head if you understand the principle.) a. 3 b. 4 c. 7 d. 11 e. 5
Read DetailsThe equilibrium 4 equation for the formation of the complex Cd(CN)42- is: Cd2+ + 4CN- ⇌ Cd(CN)42- Write the equilibrium constant expression Kf , and then answer the following question. If Cd(CN)42- is a “typical” complex (which it is), which of the following statement(s) would you expect to be true? 1. At equilibrium, there will be more Cd2+ and CN- than Cd(CN)42- 2. At equilibrium, there will be more Cd(CN)42- than Cd2+ and CN- 3. The Kf value is small (- power of 10) 4. The Kf value is large (+ power of 10) a. 2 and 4 only b. 1 and 3 only c. 1 and 4 only d. 2 and 3 only e. 2 only Tables.pdf Periodic Table with New Elements.pdf
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