a. alkali metals b. alkaline earth metals c. halogens d. noble gases e. none of the above 3. What is the collective term for the elements in Groups 1, 2, 13-18? a. actinide series b. lanthanide series c. rare earth elements d. representative elements e. transition elements 4. What is the collective term for the elements in Groups 3-12? a. actinide series b. lanthanide series
20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
A) gas B) solid C) salts D) ice E) liquid 3. A small amount of salt dissolved in water is an example of a __________. A) compound B) solid C) heterogeneous mixture D) pure substance E) homogeneous mixture 4. Which of the following is an illustration of the law of constant composition? A) Water is 11% hydrogen and 89% oxygen by mass.
If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
Litmus test: Red turned blue and blue had no reaction Dilute HCl: Fizzes and substance turns yellowish while bubbling the back to white. Dilute NaOH: Dissolves and substance became a bit thick Substance: CuCO3 Color: Green Odor: Yes Effect of Heat: Turned into black powder Solub. or Reaction w/cold H2O: No reaction. Solub. or Reaction w/hot H2O: No reaction Litmus test: No change on blue or red.
2) A compound with an empirical formula of C4H4O and a molar mass of 136 grams per mole. 3) A compound with an empirical formula of CFBrO and a molar mass of 254.7 grams per mole. 4) A compound with an empirical formula of C2H8N and a molar mass of 46 grams per mole. a. P2O3 b. C2H3 c. CH3O d. BrCl2 e. C3H4O3 f. C5H11 g. CuCO2 h. HgF 2. a. Fe3O4 b. CCl2F2 c. CH2 3. a. C5H10 b. NO2 Molecular Formula Worksheet ANSWER KEY Write the molecular formulas of the following compounds: 1) A compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole. C4O2H8 2) A compound with an empirical formula of C4H4O and a molar mass of 136 grams per mole.
If 1.40 g of N2 are used in the reaction, how many grams of H2 will be needed? ans. 0.303 g H2 4. What mass of sulfuric acid, H2SO4, is required to react with 1.27 g of potassium hydroxide, KOH? The products of this reaction are
29.4 atm B. 4.89 atm C. 25.1 atm D. 36.0 atm _____ 5. The vapor pressure of pure ethanol at 60 °C is 349 mm Hg. Calculate the vapor pressure at 60 °C of a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol. A.
(2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2. Determine the partial pressure of the hydrogen gas collected in the gas collection tube. (3 points) partial pressure H2 = total pressure - vapor pressure of water = 746mmHg - 19.8mmHg = 726mmHg 3. Calculate the moles of hydrogen gas collected. (4 points) n = 125 4.