Download Chemistry 1151, Fall 1999

Chemistry 1151, Fall 2005
NAME:________________________
Test 1A. 100 pts.
I.D.#_____________ Disc. Sec. ____
Part 1:____________
Part 1.
Part 2: ______________
Total:________________
Work must be shown for all numerical problems, or credit will not be given.
1. Write formulas for the following: (3 points each)
a. Magnesium nitrate _________________
b. Ammonium sulfide _________________
c. Potassium sulfate ___________________
d. Nickel iodide_____________________
e. Hydrobromic Acid____________________
f. Aluminum hydroxide _____________________
2. Name: (3 points each)
a. SF6
:__________________________________________
b. H2SO3(aq): an acid_____________________________________
Use the following equation for problems 3, 4, and 5.
3 Ca(OH)2(aq) + 2 Na3PO4(aq) 
Ca3(PO4)2(s) + 6 NaOH(aq)
Mol. Mass (g/mol): Ca(OH)2; 74.1, Na3PO4; 164,
Ca3(PO4)2; 310.0,
NaOH; 40.0
3. (7) If 85.00 g Ca(OH)2 are combined with 150.00 g Na3PO4, which is the limiting reactant? Answer
must be supported by calculations or explanation.
4. (7) If 48.2 g Ca(OH)2 is combined with enough Na3PO4 , how many grams of Ca3(PO4)2(s) are
produced if the yield is 73.5 %
5. (7) How many mL of 0.750 M Na3PO4 solution will react completely with 46.3 mL of 1.25 M
Ca(OH)2 solution?
6. The combustion of 3.42 g of a compound known to contain only nitrogen and hydrogen gave 9.82 g
of NO2 and 3.85 g of water.
Mol. mass(g/mol): N: 14.00; H: 1.01; O: 16.00
a. (6) Determine the empirical formula of this compound.
b. (3) If the molecular mass is 32.0 g/mol, what is the molecular formula? Support answer with
calculations.
7. (7) A metal, M, was converted to the chloride, MCl2:
M + Cl2  MCl2
A solution of MCl2 was treated with AgNO3(aq) according to the equation:
MCl2(aq)
+ 2 AgNO3(aq)  2 AgCl(s) + M(NO3)2(aq)
If 2.434 g of the metal, M, gave 7.964 g of AgCl, what is the atomic weight and the identity of the
metal?
At. Mass (amu): Ag; 107.8, Cl; 35.5, N; 14.0,
O; 16.0
Part 2. Multiple Choice:
3 points each question
_____1. Which scientist is incorrectly paired:
a. Thompson – electron,
c. Proust – neutron
b. Rutherford – nucleus of atom,
d. Dalton—Atomic Theory
_____2. What is the coefficient for oxygen when the following equation is balanced?
C4H10(g) +
O2(g) 
CO2(g) + H2O(g)
a. 7,
b. 5,
c. 10,
d. 13,
_____3. Elements A and Q form two compounds. Given the following data;
Cpd. 1: mass Q = 0.271,
Cpd. 2: mass Q = .407
Mass A
mass A
If Cpd 1 has the formula AQ, what is the formula for Cpd. 2?
a. A2Q3,
b. AQ2,
c. A3Q4,
d. AQ3,
_____4. Which of the following elements has chemical properties similar to calcium?
a. sodium,
b. nitrogen
c. hydrogen
d. strontium
_____5. How many significant figures are there in the number 0.0006042?
a. 7
b. 4
c. 8
d. 3
_____6. Convert 4.301 quarts (qts) to mL.
(1L = 1.06 qts)
a. 4.559 mL
b. 4559 mL
c. 4.058 mL
_____7.
d. 4058 mL
A transition metal, a halogen and a semi-metal in that order are:
a. Ni, N, Sn,
b. Cr, Cl, As,
c. As, Cl, Se,
d. Ca, Cl, Se
_____8. Rhenium (Re) has 2 stable isotopes and an average atomic mass of 186.2 amu. Given that
37.1% of natural rhenium is Re–185, what is the other stable isotope?
a. Re-183
b. Re-187
c. Re-189
d. Re-181
_____ 9. How many carbon atoms are there in 52.06 g of carbon dioxide?
a. 5.206x1024
b. 3.134x1025
c. 7.122x1023
d. 1.424x1024
_____10. How many protons (p) and neutrons (n) are in an atom of 3890 Sr?
a. 38 p, 52 n
b. 38 p, 90 n
c. 90 p, 38 n,
d. 52 p, 38 n
_____ 11. Which of the following compounds contains ionic bonds:
a. SiO2,
b . NI3
c. CH4
d. CaO
_____ 12. What is the mass in grams of a single chlorine molecule (Cl2) ?
a. 1.177x10-22 g
b. 2.37x1024 g
c. 70.90 g
________
13. The charge on the manganese in the salt MnF3 is
a. +3
b. +2
c. -3
d. -2
d. 5.887x10-23 g