Practice Exam 1

Topics: Oxygen, Atom, Oxide Pages: 6 (1256 words) Published: June 24, 2013
d 1.

What is the correct formula for the carbonate ion? (a) CH3COO(b) Cl(c) CO22(d) CO32(e) (COO-)2

c 2.

What is the name of Fe(OH)3? (a) (b) (c) iron hydroxide iron trihydroxide iron (III) hydroxide (d) (e) iron (II) hydroxide none of these

d 3.

From the following ionic compounds, choose the name-formula pair that is not correctly matched. (a) (b) (c) (d) (e) sodium sulfide ammonium nitrate zinc hydroxide sodium sulfate calcium oxide Na2S NH4NO3 Zn(OH)2 Na2SO3 CaO

b 4.

How many atoms of hydrogen are in 1.00 mole of water? (a) (b) (c) 6.02 x 1023 atoms 1.20 x 1024 atoms 1.81 x 1024 atoms (d) ( e) 2.41 x 1024 atoms 3.01 x 1023 atoms

a 5.

How many atoms of carbon are present in 34.5 g of caffeine, C8H10N4O2? (a) 8.57 x 1023 atoms (b) 2.68 x 1025 atoms (d) 2.09 x 1023 atoms (e) 4.83 x 1023 atoms (c) 1.08 x 1024 atoms

d 6.

What is the percent by mass of sulfur in Al2(SO4)3? (a) 9.38% (b) 18.8% (c) 24.6% (d) 28.1% (e) 35.4%

d 7.

What is the empirical formula for a compound containing 68.3% lead, 10.6% sulfur and the remainder oxygen? (a) PbSO2 (b) PbSO3 (c) PbS2O3 (d) PbSO4 (e) Pb2SO4

d 8.

A compound is known to contain only carbon, hydrogen, and oxygen. If the complete combustion of a 0.150-g sample of this compound produces 0.225 g of CO2 and 0.0614 g of H2O, what is the empirical formula of this compound? (a) C3H4 (b) CH4O (c) C3HO3 (d) C3H4O3 (e) C5H7O5

b 9.

A compound contains, by mass, 87.5% nitrogen and 12.5% hydrogen. Its molecular weight is found to be 32 g/mol. What is its molecular formula? (a) N2H6 (b) N2H4 (c) N2H5 (d) NH3 (e) NH2

e 10.

Balance the following equation with the smallest whole number coefficients. What is the coefficient for O2 in the balanced equation? C4H10 + O2  CO2 + H2O (a) 9 (b) 5 (c) 15 (d) 6 (e) 13

b 11.

The reaction of a hydrocarbon with oxygen to produce CO2 and water is called complete combustion. Write the balanced reaction for the complete combustion of heptane, C7H16, with the smallest whole number coefficients. Then choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". (a) 23 (b) 27 (c) 29 (d) 30 (e) 32

c 12.   d 13.

Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate? 2NH4NO3  (a) 6.60 mol (b) 14.0 mol (c) 26.4 mol (d) 13.2 mol (e) 18.0 mol

Acrylonitrile, C3H3N, is a molecule used to produce a plastic called Orlon. How many grams of acrylonitrile could be produced by reacting 583 g of propene, C3H6 with excess ammonia, NH3 and oxygen? 2C3H6 + 2NH3 + 3O2 C3H3N + 6H2O (a) 368 g (b) 1470 g (c) 462 g (d) 735 g (e) 583 g

e 14.

What mass of Cu(NO3)2 can be prepared from the reaction of 3.65 grams of copper with 5.16 grams of HNO3? Cu + 2HNO3  Cu(NO3)2 + H2 (a) 15.4 g (b) 10.8 g (c) 5.14 g (d) 10.3 g (e) 7.68 g

e 15.

The thermite reaction is performed using 8.6 g Fe2O3 and 1.8 g powdered Al metal. Which reactant is in excess and by how much?

Fe2O3 + 2 Al (a) Al, 0.3 g (d) Al, 1.1 g a 16.

Al2O3 + 2Fe (b) Fe2O3, 2.0 g (e) Fe2O3, 3.3 g (c) Al, 2.1 g

Calculate the molarity of a solution that contains 70.0 g of H2SO4 in 280. mL of solution. (a) 2.55 M (b) 6.84 M (c) 8.62 M (d) 9.78 M (e) 11.84 M

c 17.

A laboratory stock solution is 1.50 M NaOH. Calculate the volume of this stock solution that would be needed to prepare 300. mL of 0.200 M NaOH. (a) 2.25 mL (b) 10.0 mL (c) 40.0 mL (d) 1.00 mL (e) 0.100 mL

d 18.

If 45.0 mL of 0.250 M PbCl4 solution reacts with 20.0 mL of (NH4)2SO4 to reach the equivalence point, what is the molarity of the (NH4)2SO4? PbCl4(aq) + 2(NH4)2SO4(aq)  Pb(SO4)2(s) + 4NH4Cl(aq) (a) 0.502 M (b) 1.25 M (c) 2.25 M (d) 1.13 M (e) 0.563 M

b 19.

The number of electrons in a neutral atom of an element is always equal to the _______ of the element. (a) mass number (d)...
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