Pre-Calc – 45 Factored Quadratic Problems

 

1.       X²+4x-21   =  (x+7)(x-3)

2.       X²+6x-2  =  can’t be factored

3.       X²+8x+15  =  (x+3)(x+5)

4.       X²+9x+14  =  (x+7)(x+2)

5.       X²-11x+28  =  (x-4)(x-7)

6.       X²-10x+24  =  (x-4)(x-6)

7.       X²+3x+1  =  can’t be factored

8.       2X²-5x-3  =  (2x+1)(x-3)

9.       3X²-x-2  =  (3x+2)(x-1)

10.   3X²+7x+2  =  (3x+1)(x+2)

11.   2X²+5x+3  =  (2x+3)(x+1)

12.   10X²-3x-1  =  (2x-1)(5x+1)

13.   6X²-13x+2  =  (x-2)(6x-1)

14.   15X²-14x+3  =  (5x-3)(3x-1)

15.   2X²+7x+1  =  can’t be factored

16.   X²+16x+64  =  (x+8)²

17.   X²-6x+9  =  (x-3)²

18.   X²-49  =  (x+7)(x-7)

19.   4X²+4x+1  =  (2x+1)²

20.   9X²-12x+4  =  (3x-2)²

21.   9X²-1  =  (3x+1)(3x-1)

22.   X²+8x-5  =  can’t be factored

23.   4X²+7  =  can’t be factored

24.   6X²+17x+5  =  (3x+1)(2x+5)

25.   2X²-4x-30  =  (2x+6)(x-5)

26.   -X²+10x-21  =  (-x+3)(x-7)

27.   -3X² -15x-12  =  -3(x+4)(x+1)

28.   4X²+14x+6  =  2(2x+1)(x+3)

29.   6X²-33x+15  =  3(-2x+1)(-x+5)

30.   -4X²+10x+24  =  2(-x+4)(2x+3)

31.   12X²-3  =  3(2x+1)(2x-1)

32.   -8X²+24x-18  =  2(-2x+3)(2x-3)

33.   45X²+30x+5  =  5(3x+1)²

34.   X²+x-30=0  X=5;X=-6

35.   X²+10x+9=0    X=-1;X=-9

36.   X²-12x+32=0    X=4;X=8

37.   2X²+7x-4=0    X=1/2;X=-4

38.   3X²+8x-3=0    X=-1/3;X=3

39.   5X²+3x-2=0    X=1;X=-2/5

40.   3X²-8x+5=0    X=1;X=5/3

41.   25X²+20x+4=0    X=-2/5

42.   49X²-14x+1=0    X=1/7

43.   25X²=16    X=-4/5;X=4/5

44.   2X²-x-21=0    X=7/2;X=-3

45.   8X²+5x-4=2X²-8x+1  X=1/3;X=-5/2

Algebra 2 – Chapter 5.5

(page 287)

73. (3,2)

74. (2,-11)

75. (-8,-50)

76. (-13,-101)

77. (1.5,-4.25)

78. (-3.5,-13.25)

79. (10,20)

Algebra 2 – Chapter 5.2

(page 261)

47. (X+5)(X-5)

48. (X+2)²

49. (X-3)²

50. 4(R-1)²

51. (3s+2)²

52. (4t+3)(4t-3)

53. (7-10a)(7+10a)

54. (5b-6)²

55. (9C+11)²

56. 5(x-1)²

57. 2(9x-1)(9x+1)

58. 3(x+9)²

59. 4(2y-3)(y+5)

60. 7(4a-3)²

61. u(u+7)

62. 6t(t-6)

63. (v-1)(-v+1)

64. 2(d²+6d-8)

Algebra 2 – Chapter 3.2

18. -.62

20. x=12/7 y=1.178

22. no solution

24. x,y = 1,0

26. x=-1

28. x=5 y=1.5

30. x=2 y=.5

32. many solutions

34. x=4 y=5

36. no solution

38. x=-6 y=-14

40. x=5 y=16.25

42. x=2.375 y=1.875

44. y=1410.5857

46. y=-.3

48. many solutions

Algebra 2 – Chapter 2.7

13. f(-4) = -21

14. f(-2) = -11

15. f(0) = -9

16. f(5) = -4

17. h(1) = -9.5

18. h(-10) = -15

19. h(6) = -7

20. h(0) = -10

Algebra 2 – Chapter 2.4

27. x= -7 ; x=2

28. y=1/2 x + 4

29. y=3/2x-1/2

30. y=2x+16

31. y= -1/2x -15/2

32. y=4x+30

33. y=-x+8

34. y=-3x

35. y=3x-19

36. y=-2x+1

37. y=-7/8x +1

38. y=-3x+6

39. y=x+10

40. y=3x+6

43. y=7/2x x=8 y=28

Algebra 2 – Chapter 2.2

17. y=x+1

18. y=-3x-3 -1/3

19. x=1.7 undefined

20. falls

21. rises

22. falls

23. rise

24. horizontal

25. falls

26. rise

27. vertical

28. rise

29. fall

30. fall

31. vertical/undefined

32. B

33. C

34. D

35. A

36. greater, absolute value is steeper

37. line1

38. line2

39. line2

40. line1

41. neither ||

42. neither  | 

43. perpendicular

44. neither

45. (6,15)

Chemistry – Final Exam Study Guide

1. Name all of the diatomic elements

   H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

2. State 5 types of chemical reactions and give the general form for each.
   • Double Replacement Reaction : AB + CD → AD + CB
   • Single Replacement Reaction : A + BC → B + AC
   • Synthesis : A + B → AB
   • Decomposition: AB → A + B
   • Combustion: C_xH_X + O₂ → CO₂ + H₂O
3. Identify the following reactions:
   • Ni(OH)₂ → NiO + H₂O : Decomposition
   • Zn + 2HCL → H₂ + ZnCl₂ : Single Replacement Reaction
   • CH₄ + 2O₂ → 2H₂O : Combustion
   • 2H₂ + O₂ → 2H₂O : Synthesis
   • KI + AgNO₃ → KNO₃ + AgI : Double Replacement Reaction
4. What is a Precipitate?
   A Solid that forms from a solution in a reaction
5. Write Balanced Chemical Formulas For the following Reactions.
   • Al + Ni(CN)₂ → Ni + Al(CN)₂
   • Mg + Pb(PO₄)₄ → Pb + Mg(PO₄)₄
   • No Reaction, calcium is more reactant than zinc
   • BaO + Fe(NO₃)₃ → Ba(NO₃)₂(aq) + Fe₂O₃ (ppt)
   • Li₂CO₃ + (NH₄)₂SO₄ → Li₂SO₄ + (NH₄)₂CO₃
   • 2AlC₂H₃O₂ +Li₂O → Al₂O (aq) + LiC₂H₃O₂(aq)
   • F₂ + MnI₂ → I₂ + MnF₂
6. Define the following Terms:
   • Coefficient : number placed in front of symbol or compound to indicate how many moles of that substance are in the equation.
   • Subscript: number placed in the lower right of an element to indicate how many atoms of that element are in the equation
   • Reactant : Substances that enter the chemical reaction
   • Product: any substance produced in a chemical reaction
7. State 4 signs of a chemical change:
   • Color change
   • Fumes
   • Temperature change
   • Burning
   • Bubbling
8. When do you use the activity series and your solubility chart?
   • Activity series: for single replacement reactions
   • Solubility Chart: For Double replacement reactions
9. What is the difference between a formula unit and a molecule?
   A formula unit is the empirical formula for an ionic or covalent substance whereas a molecule is a group of atoms held together by intermolecular forces
10. What is avogadros’s number and what does it represent?
    6.02 X 10²³ particles per mole, it is the constant that represents the number of atoms of an substance are in 1 mole of that substance.
11. What is the mass of 2.5 X 10²⁴ atoms of iron?
    230 g Fe
12. How many molecules are there in 245 grams of water?
    8.18 X 10²⁴ molecules of H₂O
13. How many moles are there in 3.75 X 10²⁵ formula units of sodium chloride?
    62.3 moles
14. How many formula units are there in 2.75 Kg of Magnesium Nitrate?
    31.9 Formula Units of MgNO₃
15. What is the mass of 4.45 moles of barium sulfate
    1040g BaSO₄
16. What is the empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen?
    N₂O₅
17. Methyl Butanoate’s percent composition is 58.8% carbon, 9.8% hydrogen, and 31.4% oxygen. It’s molar mass is 102 g/mol. What is it’s molecular formula?
    C₅H₅O
18. Write empirical formula’s for the following compounds:
    • Ribose (C₅H₁₀O₅)
      CH₂O
    • Ethyl Butyrate (C₆H₁₂O₂
      C₃H₆O
    • chlorophyll (C₅₅H₇₂MgN₄O₅)
      C₅₅H₇₂MgN₄O₅
    • DEET (C₁₂H₁₇ON)
      C₁₂H₁₇ON
19. What is a hydrate?
    A hydrate is an amount of water added to a solid crystal
20. Find the formula and write the name of the following hydrate:76.9% calcium sulfate ; 23.1% water
    CaSO₄ • 2.3H₂O
21. What is the empirical formula of a compound having percent composition:
    • Carbon – 27.59%
    • Oxygen – 55.17%
    • Nitrogen – 16.09%
    • Hydrogen – 1.15%

    C₄O₃NH

22. How many oxygen atoms are in 75.5 grams of calcium nitrite?
    1.06 X 10²³ atoms of Oxygen
23. What is a mole ratio?
    Number of moles of one substance to another
24. List the steps in solving a stoichiometry problem.
    
    • write a Balanced

      Chemical Equation

25. How

    many

    grams

    of iron

    can be

    produced

    from

    12L of

    carbon

    monoxide

    gas
    Fe₂O₃ + 3CO → 2Fe + 3CO₂
    16g Fe

26. Zinc Metal Reacts with Hydrochloric acid in a single replacement displacement reaction. How many grams of zinc chloride will be produced if 14 gams of hydrochloric acid react?
    39g ZnCl
27. How Many grams

    of HCl would

    be required to

    produce 8.40

    grams of manganese

    dioxide?
    4HCl + MnO₂ → 2H₂O + MnCl₂ + Cl₂
    14.1g HCl

28. 7.36 grams of zinc is heated with 6.45 grams of sulfur.
    Assume 8Zn + S₈ → 8ZnS
    What amount of zinc sulfide will be produced? Which reactant is in excess and by how much?
    6.86g ZnS will be produced and there is 2.84g in excess
29. Hydrogen reacts with oxygen to form water. If you react 12L of oxygen with an excess of hydrogen and obtain .95 grams of water waht is your percent yield?
    5% yield

Chemistry – Chapter 3/4/5 *not sure* Mastering Concepts

29. Democratis
30. Dalton
31. Religious beliefs wouldn’t let them study and they didn’t have as much technology
32. Definite proportions, conservation of mass, all atoms are indivisible
33. The mas of the reactants equals the mass of the products
34. Electrons, J.J. Thompson, Plum pudding model
35. Different gases had different electrons (Cathode ray tube)
36. Negative 1/1840 of a hydrogen atom 0 amu
37. Mostly empty space, nucleus round, positive, small, dense
38. Didn’t account for neutrons or the empty space
39. They have an attraction
40. it goes directly from cathode to anode
41. J.J. Thompson’s plum pudding model
42. The positive charge of the nucleus
43. Protons & Neutrons
44. They are equal, and electrons are equal in a neutral atom
45. positive 89
46. Because the protons are canceled out by the electrons

Business Concepts – Chapter 8 Critical Thinking

Pgs. 123 prob. 20-23

20. I would mix between autocratic and free rein. Id give my employees who’ve worked for me for 6 months more responsibilities by allowing them to work together in a more free-rein structure were id use autocratic with my high school employees to ensure that they learn how to do the job correctly before they get to work within a free-rein structure.

21. In one day of school I used charisma to talk in front of a class, integrity to make sure other’s respect me and to gain trust, inspirational speaking to make sure my vision is comprehended and mostly prioritizing my goals to make sure important things get done and less important things that can wait, get done later.

22. A Chief knowledge Officer would be beneficial to a company in that, they facilitate communications and connections between employees as well as providing a company with a strong knowledge base enabling them to have a sturdy framework for their decisions.

23. Between now and the year 2020 CEO’s of companies are more likely to place greater emphasis on teams and consensus because it allows worker to be more open and let their true potential shine out, and this makes the overall product better and makes employee’s motivation higher.