HOMEWORK # 6. Ch.3.1, Ch.4.1-2. Use 2 decimal places for atomic masses. SHOW YOUR CALCULATIONS!
1. Calculate the molecular or formula mass of each of the following:
(a) P4

(b) Ca(NO3)2

2. Calculate the molar mass of each of the following compounds:

(a) silver sulfate, Ag2SO4

(b) boric acid, B(OH)3

3. Determine the number of moles of compound and the number of moles of each type of atom in the following: 0.325 g of aspirin, C6H4(CO2H)(CO2CH3).

4. A 55-kg person has 7.5 × 10–3 mol of hemoglobin (molar mass = 64,456 g/mol) in the blood. A) How many hemoglobin molecules is this?
b) What is this quantity in grams?

5. Balance the following equations and classify the type of the reactions:

(a)
b)

6. Write a balanced equation describing each of the following chemical reactions, indicate
physical state of substances and type of the reactions:

(a) Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6.
(b) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and
aqueous sodium sulfate are produced.

7. Complete and balance the following equation, indicate physical state of substances and type of
the reaction: Aqueous H2SO4 reacts with aqueous NaOH

12 is probably the typical age for a first kiss but i think its to young.

1.75 is the weight of one medium egg

  remember that hf is only the energy of one photon. not two. not three. one.  1) 5.12 * 10^3 photons  find the energy of one photon, then determine how many photons are needed to reach the sensitivity.  e = hf  = (6.626 * 10^-34 js)(5.95 * 10^19 hz)  = 3.94247 * 10^-14 j per photon  (2.02 * 10^-10 j) / (3.94247 * 10^-14 j/photon) = 5123.69149 photons  round to three sig figs.  2) 5.77 * 10^-17 j  energy of pulse = energy per photon * number of photons  = hfn  = (6.626 * 10^-34 js)(1.66 * 10^13 hz)(5250)  = 5.774559 * 10^-17 j  round to three sig figs.  3) 4.07 * 10^8 kj/mol  10^12 pm = 1 m  c = fλ  f = c/λ  e = hf  = hc/λ  = [(6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.94 * 10^-12 m)](1 kj/1000 j)(6.02 * 10^23 photons/mol)  = 40702571.4 kj/mol  round to three sig figs.  4) 9.94 * 10^-1 m  e = hc/λ  λ = hc / e  = (6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.00 * 10^-25 j)  = 0.9939 m  round to three sig figs.  5) 9.06 * 10^3 photons  energy of pulse = energy per photon * number of photons  number of photons = energy of pulse / energy per photon  = energy of pulse / (hf)  = (3.87 * 10^-13 j) / [(6.626 * 10^-34 js)(6.45 * 10^16 hz)]  = 9055.23695 photons  round to three sig figs.  6) 2.78 * 10^-15 j  this is problem 1, except in reverse.  sensitivity = minumum number of photons * energy per photon  = (5930)(6.626 * 10^-34 js)(7.077 * 10^14 hz)  = 2.78070758 × 10^-15 j  round to three sig figs.