Chemistry Chapter 4
What volume of a 0.540 M NaOH solution contains 11.5 g of NaOH?
0.532 L
The mixing of which pair of reactants will result in a precipitation reaction?
Ba(NO3)2(aq) + Na2CO3(aq)
Which of the following compounds is an Arrhenius base?
CsOH
Which of the following is not a strong electrolyte?
MgCO3
How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl?
2.96 L
How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s)
20.3 g Li3N
How many of the following compounds are soluble in water? Cu(OH)2 LiNO3 NH4Br K2S
3
Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
3.50 moles O2
How many milliliters of 0.550 M hydriodic acid are needed to react with 15.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)
5.92 mL
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?
51.1
How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?
7.65 × 10-3 mol
Define a strong electrolyte.
A substance that dissolves in water to form a solution that conducts electricity.
Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
K+ & NO3-
The mixing of which pair of reactants will result in a precipitation reaction?
K2SO4(aq) + Hg2(NO3)2(aq)
Determine the oxidation state of P in PO3 3-.
+3
Determine the oxidation state of Sn in Sn(SO4)2.
+4
Give the oxidation state for S in SO3-2.
+4
Determine the oxidation state of Cl in NaClO3.
+5
What is the oxidation number of the chromium atom in Na2CrO4?
+6
What is the oxidation number of the sulfur atom in Li2SO4?
+6
Determine the oxidation state of Mn in KMnO4.
+7
What is the oxidation number of the oxygen atom in Rb2O2?
-1
What is the oxidation number change for the bromine atom in the following unbalanced reduction half reaction: BrO3 -(aq) + H+(aq) → Br-(aq) + H2O(l)?
-6
What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?
.29
How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas? 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l)
0.00197 g
How many moles of CO2+ are present in 0.150 L of a 0.200 M solution of CoI2?
0.0300
Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL.
0.0313 M
Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.
0.0337 M
Which of the following solutions will have the highest electrical conductivity?
0.045 M Al2(SO4)3
Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N2(g) → 2Li3N(s) . How many moles of N2 are needed to react with 0.500 mol of lithium?
0.0833
What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq).
0.0833 M
How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH)3(aq)
0.0914 mol
Which of the following solutions will have the highest concentration of chloride ions?
0.10 M AlCl3
A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution?
0.108 g
The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)?
0.114 M
A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?
0.117
Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.
0.126
Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen?
0.150
If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?
0.162 M
Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction. 2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)
0.187 g
In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?
0.194 M
Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
0.198 g CO2
1.06g of Na2CO3 is dissolved in 100mL of water. What is the molarity of Na+ ions in the solution?
0.2 M
The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)?
0.20 M
What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?
0.250 M
A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?
0.274 M
Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL.
0.350 M
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns in excess oxygen?
0.385
What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough water to make 275 mL of solution?
0.448 M
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq) + Cl-(aq) → AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 M AgNO3 solution to completely precipitate the silver?
0.535 g
If 100. mL of 0.400 M Na2SO4 is added to 200. mL of 0.600 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.
0.667 M
A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.
0.675
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4mol NO2 and 2 H2O mol combine and react completely. How many moles of the reactant in excess are present after the reaction has completed?
0.7
How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
0.724 mol O2
A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.
0.747
How many moles of NaCl are required to make 250 mL of a 3.00 M solution?
0.750 moles
What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
0.801
What mass, in g, of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)
0.838 g
What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?
1.02 M
When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq)
1.07 g
Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.250 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l).
1.12 M
How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)
1.12 g
What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na3P solution?
1.19
How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution?
1.21 × 1021 molecules C12H22O11
What is the concentration of ions in a 0.25 M Al2(CO3)3 solution?
1.25 M
Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4 mol NO2 and 2 H2O mol combine and react completely. How many moles of NO are produced after the reaction has completed?
1.33
There are ________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.
1.35
What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution?
1.35 M
Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.
1.50 M
According to the balanced equation shown below, 4.00 moles of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l)
1.60
When 7.00 × 1022 molecules of ammonia react with 6.00 × 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)
1.63 g
Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ____ Al(s) + ____ I2(s) → ____ Al2I6(s)
1.67 mol
Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?
1.8
How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction? 2 Cu2O(s) + O2(g) → 4 CuO(s)
1.80 mol
According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)
1.99 × 10-2 moles
Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
10.9 g H2O
According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
10.9 moles H2O
According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
10.9 moles H2O
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq)
102 mL
Give the theoretical yield, in grams, of CO2 from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
112.7 g
If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 32.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
126 g
How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.35 L of a 3.5 M solution?
140 mL
Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide. ____ Ca(OH)2(aq) + ____ H3PO4(aq) → ____ Ca3(PO4)2(aq) + ____ H2O(l)
15.0 mL
If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2
160
A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed?
17.01 g
According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
17.22 g
How many H+ ions can the acid, H2SO4, donate per molecule?
2
How many of the following compounds are insoluble in water? KC2H3O2 CaSO4 SrS AlPO4
2
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.
2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed.
2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)
Which of the following is an acid base reaction?
2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed.
2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)
Which of the following is a precipitation reaction?
2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq)
What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ____ NO3-(aq) + ____ Cu(s) → ____ NO(g) + ____ Cu2+(aq)?
2, 3
Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
2.0 mol H2S
What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?
2.28
How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution?
2.48 × 1022 chloride ions
Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
2.56 moles
How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?
2.75
How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl
2.78 × 1024 molecules HCl
According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
2.81 moles NO
What is the concentration of an AlCl3 solution if 150. mL of the solution contains 450. mg of Cl- ion?
2.82 × 10-2 M
Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many grams of water remain after the reaction is complete?
2.90
How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?
22.5 mL
How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s)
24.2 mL
When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g)
24.6%
Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the chemical equation: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq).
24.9 mL
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
25.00%
A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make 450. mL of a solution that is 0.300 M in Cl- ion?
257 mL
What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: you will want to write a balanced reaction.
278 mL
How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M
29.9
According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2. 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
3.59 g
Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?
3.64 g
If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
30.8 g
Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a 0.7450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2+(aq) + Sn4+(aq).
33.58%
How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?
39.0
Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+(aq) + 2I-(aq) → PbI2(s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of Pb(NO3)2(aq) to completely precipitate the lead?
394 mL
Methane (CH4) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). (See figure on test #193)
4
Methane (CH4) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). (See figure on test #194)
4
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?
4.32
How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution?
4.32 × 10-2 mol
Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H2CO3 → H2O + CO2
4.40 g
Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?
4.68 g
How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution?
42.3 mL
How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M NaNO3 solution?
42.3 mL
How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution?
43.83 g
What mass of N2 will be produced from the reaction of 50.0 g N2O4 with 45.0 g N2H4? N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
45.7 g
How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
49.7 g O2
What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L?
5.2 M
Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.
5.30
How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 M?
5.73 g
Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) In a particular experiment, 3.50 g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g.
5.85
A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed?
54.93 g
Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol. BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
56.0 g HCl
How many grams of H2 gas can be produced by the reaction of 54.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below? 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)
6.05 g
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
6.63
How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3?
614 mL
What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution?
69.4 mL
Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ____ NH3(g) + ____ O2(g) → ____ NO(g) + ____ H2O(l)
7.32 L
Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3 . ____ MgO(s) + ____ Fe(s) → ____ Fe2O3(s) +_____ Mg(s)
7.57 g
How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution?
8.28 × 1021 aluminum ions
When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride?
8.44 g
Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)
81.93%
According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
86.1 mL
How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH?
9.6
How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2. 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
9.89 × 1023 molecules H2S
If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)
9.95 mL
Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2 is recovered. What is the percent yield in this experiment?
92.5
According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
99.8 g S
Describe the difference between complete ionic and net ionic equations.
A complete ionic equation shows all of the substances present in the reaction mixture. A net ionic equation only shows the substances that are participating in the reaction. The spectator ions are absent in the net ionic equation.
Define a net ionic equation.
A net ionic equation is an equation showing only the species that actually change during the reaction.
What causes a precipitation reaction to occur between two soluble compounds?
A precipitate, or insoluble compound, forms from a pair of the ions present that participate in a reaction. This "traps" some of the ions into a newly formed compound causing reaction.
Explain the difference between a strong and weak electrolyte. Give an example of each.
A strong electrolyte is either an ionic compound that is soluble in water or a molecular compound that ionizes completely in water. Possible examples are NaCl or HCl. A weak electrolyte is only slightly soluble or does not ionize to any great extent in water. Possible examples are AgCl or HC2H3O2.
Choose the statement below that is true.
A weak acid solution consists of mostly nonionized acid molecules.
Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
Ag
What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
Ag
What is the net ionic reaction for the following reaction in aqueous solutions: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Ag+(aq) + Cl-(aq) → AgCl(s)
What reagent could be used to separate Br- from CH3CO2 - when added to an aqueous solution containing both?
AgNO3(aq)
What reagent could not be used to separate Br- from CO3 2- when added to an aqueous solution containing both?
AgNO3(aq)
Which of the following pairs of aqueous solutions will produce a precipitate when mixed?
All of these solution pairs will produce a precipitate.
How can you tell if a reaction is an oxidation-reduction reaction?
At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by assigning oxidation numbers to each element present and looking to see if these change from reactant to product.
What precipitate is most likely formed from a solution containing Ba+2, Na+1, OH-1, and CO3-2.
BaCO3
What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
C
Which substance is oxidized in the following reaction? 5C2O42- + 2MnO4- + 16H+ → 10 CO2 + 2Mn2+ + 4H2O)
C2O42-
Choose the reaction that represents the combustion of C6H12O2.
C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g)
Which of the following compounds is an Arrhenius base?
C6H5NH2
Which of the following is not a strong electrolyte?
CH3CH2CH3
Which of the following compounds is not an Arrhenius acid?
CH3CH2NH2
Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI, behave as bases when they are dissolved in water?
Ca(OH)2 and KOH
Which of the following compounds is soluble in water?
CaS
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed.
Fe2+(aq) + S2-(aq) → FeS(s)
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed.
H+(aq) + OH-(aq) → H2O(l)
Which of the compounds of H2C2O4, Ca(OH)2, KOH, and HI, behave as acids when they are dissolved in water?
H2C2O4 and HI
Which one of the following compounds behaves as an acid when dissolved in water?
HI
Which of the following pairs of aqueous solutions will react to produce a precipitate?
Hg2(NO3)2 + LiI
Which of the following compounds is insoluble in water?
Hg2I2
Sodium metal reacts with oxygen to form sodium oxide according to the reaction: 4 Na(s) + O2(g) → 2 Na2 O(s) A flask contains three oxygen molecules. Which image best represents the amount of sodium required to completely react with all of the oxygen in the flask? (See figure on test #192)
III
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
LR = N2O4, 45.7 g N2 formed
Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s)
Li
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed.
Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)
Which of the following is an oxidation-reduction reaction?
Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
Which statement is correct for the following redox reaction? 5 Fe2+ + MnO4- +8H+ → 5 Fe3+ +Mn2+ + 4H2O
MnO4- is the oxidizing agent.
Which of the following is a gas-evolution reaction?
NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)
Which of the following is considered a strong electrolyte?
NH4NO3
What are the spectator ions for the following reaction in aqueous solution: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Na+ & NO3 -
List the spectator ions in the following reaction. Ba+2(aq) + 2 OH-(aq) + 2 Na +(aq) + CO3-2(aq) → 2 Na +(aq) + 2 OH-(aq) + BaCO3(s)
Na+ and OH-
Which pair of compounds is soluble in water?
NaI and Cu(NO3)2
Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l)
NaOH(aq)
Methane (CH4) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). (See figure on test #195)
O2
Which one of the following compounds is insoluble in water?
Pb Cl2
Which one of the following compounds is soluble in water?
Pb(NO3)2
Which of the following pairs of aqueous solutions will react to produce a precipitate?
Sr(C2H3O2)2 + Na2SO4
How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days. Why?
The concentration would slowly increase as water from the solution evaporated. This is because the amount of NaCl in the flask would remain constant while the amount of water decreases.
7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is FALSE? N2(g) + 3 H2(g) → 2 NH3(g)
The theoretical yield of ammonia is 15 g.
5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which one of the following statements is FALSE? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)
Water is the limiting reactant.
When dissolved in water, KOH behaves as
a base that forms K+ and OH- ions.
When 280. mL of 1.50 × 10-4 M hydrochloric acid is added to 135 mL of 1.75 × 10-4 M Mg(OH)2, the resulting solution will be
basic
HCl , HI , H2SO4, LiCl , and KI are all classified as
strong electrolytes.
