Chemistry Test #3 Study Guide
How many moles are in each of the following? 16 grams of H2O 24 grams of HCl 245 grams of C13H18O2 102 grams of CH3CH2OH
0.89 mole H2O 0.66 mole HCl 1.19 mol C13H18O2 2.22 mol CH3CH2OH
How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown? 2 Fe + 3 F2 → 2 FeF3
10.1g F2
How many grams of Ag are produced when 5.72 g Cu react according to the following equation? Cu (s) + 2 AgNO3 (aq) → 2 Ag (s) + Cu(NO3)2 (aq)
19.4 g Ag
Complete each of the following double-replacement reactions, including their states, and write the net ionic equation for each. a) K3PO4(aq) + Al(NO3)3(aq) → b) AgNO3(aq) + KCl(aq) → c) Mg(NO3)2(aq) + Na2CO3(aq) → d) HBr(aq) + NaOH(aq) →
240325.pdf from Abby's email on Wed 3/27/2024
Determine the oxidation states of each element: a) NaNO3 b) NH3 c) ZnO d) H2O e) CaH2 f) CO2 g) N2 h) Na2SO4 i) Al(OH)3 j) Mg3(PO4)2
240325.pdf from Abby's email on Wed 3/27/2024
How many grams are in 1.25 moles of Ne?
25.2 g Ne
Using the reaction shown, if you start with 2.00 grams of each, which will run out first? ____ AlBr3 + ____ K2SO4 → ____ KBr + ____ Al2(SO4)3
2AlBr3 + 3 K2SO4 → 6KBr + Al2(SO4)3 2.00 g AlBr3= 0.0225 molKBr 2.00 g K2SO4= 0.0230 molKBr AlBr3 will run out first
For the following reaction, if 11.2 L of nitrogen are reacted to form NH3 at STP, How many liters of hydrogen will be required to completely consume all of the nitrogen?N2 + 3H2 → 2NH3 33.6 L 11.2 L 7.4 L 16.8 L 6.1 L
33.6L
For the reaction given below, what quantity of heat will be produced if 90.0 g of C3H8 are consumed in the reaction?C3H8 + 5O2 --> 3CO2 + 4H2O + 488 kcal 996 kcal 488 kcal 332 kcal 239 kcal 976 kcal
488 kcal
What volume will be occupied by 8.00 g of oxygen, O2, at STP? 4.00 L 11.2 L 13.4 L 22.4 L 5.60 L
5.60 L
Consider the reaction shown:N2 + O2 → 2 NO ΔH = +43.2 kcalWhen 50.0 g of N2 react, ________ kcal will be ________. 77.1; consumed 2160; produced 2160; consumed 43.2; produced 77.1; produced
77.1; consumed
When copper (II) hydroxide reacts with phosphoric acid (H3PO4) to form water and solid copper (II) phosphate, how many grams of phosphoric acid are needed to completely react with 13.40 g of copper (II) hydroxide?
8.973 g H3PO4
Reduction is the process of gaining electrons. losing oxygen. gaining hydrogen. forming an anion from a neutral atom. all of the above
All of the above
In the reaction shown, ________ is the oxidizing agent because it ________.Ni (s) + CuCl2 (aq) → Cu (s) + NiCl2 (aq) CuCl2; gets reduced Ni; causes reduction CuCl2; causes reduction NiCl2; gets reduced Ni; gets reduced
CuCl2; gets reduced
Using the reaction shown, if you start with 8.21 g of calcium nitrate and 7.34 g of sodium phosphate, how much sodium nitrate will be formed? What is the limiting reagent? 3 Ca(NO3)2 + 2 Na3PO4 → Ca3(PO4)2 + 6 NaNO3
How much sodium nitrate will be formed? 0.100 mol What is the limiting reagent? Ca(NO3)2
In the following reaction, list which elements are oxidized and reduced, and which compounds are the oxidizing and reducing agents. 2KrF2 + 2H2O → 2Kr + 4HF + O2 Oxidized: Reduced: Oxidizing Agent: Reducing Agent:
Oxidized: Reduced: Oxidizing Agent: Reducing Agent:
For the following reaction, determine what is oxidized and reduced, and what the reducing and oxidizing agents are 2 NaCl + F2 → 2 NaF + Cl2 Oxidized: Reduced: Oxidizing agent: Reducing agent:
Oxidized: Reduced: Oxidizing agent: Reducing agent:
What is the pressure of a 1.09 g sample of H2 gas contained in a 2.00 L container at 20.0°C?
P= 6.51 atm
Lead (II) nitrate combines with potassium chromate to form potassium nitrate and solid lead chromate. Write and balance the equation.
Pb(NO3)2 + K2CrO4 --> 2KNO3 + PbCrO4
Which of the following might be insoluble in water? Select all that apply. PbCl2 PbSO4 Ba(NO3)2 (NH4)2S KI BaSO4 HNO3 AgBr
PbCl2 PbSO4 BaSO4 AgBr
How many moles of sulfuric acid are required to react with 7.43 moles of sodium acetate? ____ H2SO4 + ____ NaC2H3O2 → ____ Na2SO4 + ____ HC2H3O2
_H2SO4 + 2 NaC2H3O2 → Na2SO4 + 2 HC2H3O2 3.72 mol H2SO4
Which of the following are not soluble in water? Select all that apply. a. KNO3 b. Pb(NO3)2 c. Cu(OH)2 d. NaCl e. AgCl f. PbI2
c, e, f
Determine what is oxidized and what is reduced for each reaction. Identify the oxidizing agent and the reducing agent. e) 2Cs + Br2 → 2CsBr Oxidized: Reduced: Oxidizing agent: Reducing agent: f) 3Mg + N2 → Mg3N2 Oxidized: Reduced: Oxidizing agent: Reducing agent: g) 4Fe + 3O2 → 2Fe2O3 Oxidized: Reduced: Oxidizing agent: Reducing agent:
e) 2Cs + Br2 → 2CsBr Oxidized: Cs Reduced: Br2 Oxidizing agent: Br2 Reducing agent: Cs f) 3Mg + N2 → Mg3N2 Oxidized: Mg Reduced: N2 Oxidizing agent: Mg Reducing agent: N2 g) 4Fe + 3O2 → 2Fe2O3 Oxidized: Fe Reduced: O2 Oxidizing agent: O2 Reducing agent: Fe
When a solution of iron(III) nitrate is mixed with a solution of sodium hydroxide, a rust colored precipitate forms. This precipitate is probably iron (III) hydroxide. sodium hydroxide. sodium nitrate. iron (III) nitrate. none of the above
iron (III) hydroxide.
Classify each of the following reactions as either redox, acid-base neutralization, or precipitation reaction a. BaCl2 (aq) + K2SO3 (aq) → BaSO3 (s) + 2 KCl (aq) b. Fe3O4 (s) + 4 H2 (g) → 3 Fe (s) + 4 H2O (l) c. H2SO4 (aq) + Ca(OH)2 (aq) → CaSO4 (aq) + 2 H2O (l)
precipitation redox acid base
How many grams of carbon will be consumed when 5.00 grams of Na2SO4 react according to the reaction shown? Na2SO4 + 2 C → Na2S + 2 CO2
0.0846 g C
Determine what is oxidized and what is reduced for each reaction. Identify the oxidizing agent and the reducing agent. a) 2C2H2 + 5O2 → 4CO2 + 2H2O Oxidized: Reduced: Oxidizing agent: Reducing agent: b) Cu + HNO3 → CuNO3 + H2 Oxidized: Reduced: Oxidizing agent: Reducing agent: c) 2Sr + O2 → 2SrO Oxidized: Reduced: Oxidizing agent: Reducing agent: d) 2Li + S → Li2S Oxidized: Reduced: Oxidizing agent: Reducing agent:
a) 2C2H2 + 5O2 → 4CO2 + 2H2O Oxidized: C2H2 Reduced: O2 Oxidizing agent: O2 Reducing agent: C2H2 b) Cu + HNO3 → CuNO3 + H2 Oxidized: Cu Reduced: HNO3 Oxidizing agent: HNO3 Reducing agent: Cu c) 2Sr + O2 → 2SrO Oxidized: Sr Reduced: O2 Oxidizing agent: O2 Reducing agent: Sr d) 2Li + S → Li2S Oxidized: Li Reduced: S Oxidizing agent: S Reducing agent: Li