Assignment:
Answer the questions and show your work in the space provided.
Question 1. Convert the following numbers to standard exponential form:
a) 0.003621 ________________ b) 0.0847 __________________
c) 15 4 ____________________ d) 536.2 x 103 _______________
Question 2. How many significant figures are there in the following:
a) 0.0549 __________________ b) 10.64 _______________
c) 60204 __________________ d) 357.9 x 105 _______________
Question 3. Add or subtract as indicated. Express to the proper number of significant figures.
a) 18.20 + 0.005 + 6.321 = __________ b) 6.42 + 4.41 - 64 = _________
c) 600 - 107.6 = _________ d) 75.2 + 145 - 75.03 = _________
Question 4. Multiply or Divide the following problems. Round to the correct number of significant figures.
a) (64.69)(8.08) = _____________ b) 0.7406/0.144 = _____________
c) (354.43)(4.596) = _____________ d) 345.67/9.01 = _____________
Question 5. Write the names of the chemicals shown by their formulas/or the formulas from the given names.
a) BaCl2 ____________________ b) KMnO4 ___________________
c) H2SO4 ____________________ d) H2O ___________________
e) AgNO3 ____________________
f) sodium hydrogen carbonate _________________
g) nitric acid _________________
h) hydrochloric acid _________________
i) potassium dichromate _________________
j) sodium hydroxide _________________
Question 6. Complete the following conversion factors or problems:
a) 1 cm3. = ______ mL. 1 kg. = ________ g. 10 cm. = _______ mm.
b) convert 6.54 ft to centimeters:
c) convert 1.20 pounds to milligrams: (Use scientific notation for your final answer).
Question 7. Write a balanced chemical equation to represent each of the following reactions:
a. The decomposition, by heating, of solid mercury(II) nitrate to produce pure liquid mercury, nitrogen dioxide gas, and oxygen gas.
b. The reaction of aqueous potassium hydroxide with aqueous hydrochloric acid (hydrogen chloride) to produce water, and aqueous potassium chloride.
Question 8. Calculate the formula weight (molar mass) of LiC2H3O2.
Question 9. Calculate the mass of 0.250 moles of LiC2H3O2.
Question 10. In an experiment to test how well methyl alcohol works as an antifreeze, a technician collected a sample of 175.0 mL of this liquid. Its density is 0.810 g/mL. How many grams of methyl alcohol were taken?
Question 11. A sample of substance X weighs 115.9 g. Initially at a temperature of 23.5 oC, its temperature rises to 58.6 oC. If substance X is found to have a heat capacity of 0.215 cal/g oC, how much heat was absorbed by the substance?
Question 12. Balance the following equations by inspection. Mark the correct coefficient in the space provided. NOTE: While we normally do not write coefficients which equal one in a chemical equation, please do so.
a. ____ Mg + ____ O2 →____ MgO
b. ____ CaBr2 + ____ H3PO4 → ____ Ca3(PO4)2 + ____ HBr
c. ____ Al(OH)3 + ____ HNO3 → ____ Al(NO3)3 + ____ H2O
d. ____ C4H10 + ____ O2 → ____ CO2 + ____ H2O
e. ____ Al + ______ HCl → _____ AlCl3 + _____ H2
Provide complete and step by step solution for the question and show calculations and use formulas.