Name __________________________________________________________________________________ Spring Final Review Chapter 10: The Mole 1.
Solve the following problems: a.
86.5 g Cu = _________ moles Cu = ___________________________atoms of Cu b.
5903 grams of Cl = ____________ moles of Cl c.
9.0 moles HF = _______ grams of HF d.
5.00x 1028 atoms of Zn = ______________ grams of Zn (2 steps) 2.
What is the percent composition of each element in Al(OH)3? 3.
Give an example of an empirical formula and a molecular formula. How are they different from each other? 4.
What are the empirical and molecular formulas of a compound that is 5.935% hydrogen and 94.1% oxygen and has a molar mass of 34.01 g/mol? Chapter 11: Stoichiometry 5.
Hydrochloric acid is neutralized by aluminum hydroxide in the following equation: Al(OH)3 + 3HCl  AlCl3 + 3H2O a) How many moles of Al(OH)3 are needed to neutralize 1.5 moles of HCl? b) If 3 grams of Al(OH)3 are used, how many grams of AlCl3 would be produced? Chapters 12: States of Matter 6.
Name the factors which affect the rate of a solute dissolving and describe how they work. a.
____________________ ________________________________________________________________ b.
____________________ ________________________________________________________________ c.
____________________ ________________________________________________________________ Chapter 13: Gas Laws 7.
What are STP conditions? T = _____K or _____oC 8.
To convert degrees Celsius to Kelvin, _________________________________ 10oC = ___________K 9.
P = ______ kPa or ____ atm or _____ mm Hg 465 K = ___________°C 85oC = _________ K As pressure of a gas increases, volume___________________________ (if temperature is constant). As temperature increases, volume __________________________ (if pressure is constant). As volume increases, temperature _____________________________ (if pressure is held constant). 10. The pressure of 100 mL of gas changes from 102 kPa to 97.9 kPa, what is its new volume? 11. What is the pressure of a gas at 98 kPa that changes from 70°C to 85oC as its volume changes from 5L to 18 L? 12. To change the volume of a gas at constant temperature from 5.00L to 2.00L, it would be necessary to change the pressure from 5.5atm to _____________ if the temperature is held constant. Chapter 14: Solutions 13. What is the molarity of a solution that has 48 moles of HCl in 4 liters of solution? 14. How many grams of KCl are needed to make 3.0 L of a 3.4 M solution? 15. Calculate the % concentration by mass of a solution prepared when 10 g of solute is added to 50 grams of water. 16. Define: a.
solute ______________________________________________________________________ b.
solvent ______________________________________________________________________ c.
solution ______________________________________________________________________ d.
solubility ______________________________________________________________________ 17. Identify each solution as saturated, supersaturated or unsaturated: a.
40g NaCl at 20 oC ______________________ b.
60g of KNO3 at 40 oC ______________________ c.
20g of KClO3 at 80 oC ______________________ d.
80g of NaNO3 at 10 oC ______________________ 18. If KCl is cooled from 80 oC to 10 oC, how much will precipitate out of solution? Chapter 15 Energy and Change and Chapter 16 Reaction Rates 19. Temperature is a measure of the average ____________ _____________ of the particles. 20. Heat is a measure of _________________________. Heat flows from __________areas to _________areas. 21. Define specific heat capacity______________________________________________________________ 22. Define activation energy: ____________________________________________________________ 23. During an exothermic reaction, the products have ( less OR more ) energy than the reactants. During an endothermic reaction, the products have ( less OR more ) energy then the reactants. Chemical reactions that use energy are _________________ while those that produce energy are ______________. 24. Draw energy diagrams showing endothermic and exothermic curves and label the following: Time
Energy Activation Energy (Ea) Enthalpy Reactants (R) Products (P) Activated complex 25. To find heat energy (q), you would use the formula: __________________________________________ 26. What is the specific heat of water in J/g°C? ______________ in cal/g°C? ______________ 27. How much heat is needed to change the temperature of 100 g of water from 20°C to 42°C? 28. 500 J of heat energy was applied to 10 g of aluminum (specific heat = 0.215 J/g°C). What was its temp. change? 29. Name the factors which affect the rate of a chemical reaction. a.
_______________________________________ c.
_______________________________________ b.
_______________________________________ d.
_______________________________________
30. How does a catalyst affect reaction rate? __________________________________________________________ Chapter 19 Acids, Bases, and Salts 31. Put an “A” under the acids, a “B” under the bases, and an “S” under the salts: HCI H3PO4 Al(OH)3 NaOH HF NaF HC2H3O2 NH4OH HClO3 CaO 32. According to Arrhenius, acids produce______________ and bases produce ______________in water while Brønsted‐Lowry defined acids as ______________ donor and bases as _______________ acceptors. 33. Complete the chart for characteristics of acids and bases. Each property may apply to one, both or neither. 34. State the formula for solving for pH: _______________________________ 35. pH + pOH = _______ If pH=6.5 then pOH = _______ 36. What is the pH of a HCl solution with a [H+] of 1.0 x 10‐6M? _______________________ 37. If the pH is 8 then the [H3O+] = _____________ If the pH is 5 then the [H3O+] = _____________ 38. Acids and bases neutralize to form __________ and _____________. 39. NaCl + KOH ‐‐‐ __________ + ________ (Hint: this is a neutralization reaction)