1 For the hypothetical reaction A+B=> products, the rate law is first order in A and first order in B. When the initial concentrations of A and B are .05 M and .08 M respectively, the initial rate is 1.6x10^-3 M/s.

a) What is the form of the rate equation? b) What is the value and units of the rate constant? c) If the initial concentration of A were tripled what would happen to the rate? d) If the initial concentration of A and B were both tripled what would happen to the rate? e) If the initial concentration of A and B were both tripled what would happen to the rate constant? f) What would the initial rate be if the initial concentrations of A and B are .035 M and .098 M? respectively

2. a) At 215 C the rate of decomposition of CH₃CN is first order with a rate constant of 2x10 ^-4 sec ^-1 . What is the half life of CH₃CN at this temperature? (Answer = 3.5x10 ³ sec) b) How much time would it take for 16 g of CH₃CN to decompose so that only 1 gram remains? (Answer= 3.9 hours)

3.The following data are collected for the gas phase reaction:

NO + 1/2 Br₂ = NOBr

a) What is the rate law and explain how you know.b) Calculate the value of the rate constant. (including units)c) What would be the initial rate if the concentration of NO is 0.4 and of bromine is 0.5?

ans b 12000 M^-2s^-1 

4. Which of the following is most likely to be bonded covalently? Explain

a) K₂S b) SiH₄ c) BaCl₂ d) FeO e) ZnF₂

5. 23.7 grams of Ca(CN)₂ = _________moles of Ca(CN)₂? Moles of CN? Moles of Ca?

6. Define the following terms paying particular attention to distinguishing between them:

rate, rate equation, rate constant.

7.  express log(a^m) without using an exponent.

8.  express log(a/b) with out using the division sign.

9.  8= 2^x.  what is x?

10.  14.3