Chemistry 102 : Can You Pass This Trivia Test? Quiz

30 Questions | By Catherinehalcomb | Last updated: Mar 20, 2022 | Total Attempts: 148

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Are you taking chemistry 102? Can you pass this trivia test? One of the keys to understanding everything you are taught in chemistry class is to have adequate knowledge on the different chemical elements in existence and the different changes exhibited when they interact and the formulas as well. Take the test and stand a chance at refreshing your memory on what you have learnt so far. All the best!

Questions and Answers

1.

Calculate the concentration of CO₂, P= 3*10^-4 atm , if the K=3.4*10^-2 M/atm.
- A.
  
  16*10^-7
- B.
  
  10*10^-6
- C.
  
  11*10^-6
- D.
  
  17*10^-7
2.

If the molar mass of glucose is 180g/mol, the solubility of glucose in the water at 20⁰c is 30g/100ml is a 1.22M solution of glucose at 20⁰c:
- A.
  
  Saturated
- B.
  
  Unsaturated
- C.
  
  Super saturated
- D.
  
  None
3.

2M solution of Nicl2 has a density of 2.18Kg/ml, calculate the molality if ( M.m=129.7g/mol)?
- A.
  
  9*10^-3m
- B.
  
  9.175*10^-4 m
- C.
  
  8.1*10^-4m
- D.
  
  9.9*10^-4m
4.

The vapor pressure of water at 110⁰c is 1070 torr, a solution of ethylene , and water has a vapor pressure of 1atm , what is the mol fraction of ethylene?(1atm=760 mmHg = 760 torr)
- A.
  
  0.71
- B.
  
  0.55
- C.
  
  0.29
- D.
  
  0.77
5.

Calculate the freezing point and boiling point of solution made of 25% by mass of CH₂OHCH₂OH (62 g/mol) in water give that (Kf of H₂O=1.86) (Kb of H₂O=0.5)
- A.
  
  -9.92 , -102.72
- B.
  
  -9.92,102.72
- C.
  
  9.92, 102.72
- D.
  
  9.92, -102.72
6.

2NO₂-----> 2NO+O₂ has a rate constant K=0.63 M^-1 S^-1, IF [NO₂]=0.1 M, what is the half life ?
- A.
  
  15.8
- B.
  
  15.0
- C.
  
  16
- D.
  
  16.1
7.

Ea= 65.7 KJ/mol, how many times faster the rxn will occur at 50⁰c to 0⁰c?
- A.
  
  77.32
- B.
  
  88
- C.
  
  88.234
- D.
  
  90
8.

2N₂O₅------> 4NO₂+O₂, and (K=6.82 S^-1) we stated with 0.025 mol in 2 L, How many moles of N₂O₅ will remain after 5 min?
- A.
  
  3.232*10^-3mol
- B.
  
  4*10^-2 mol
- C.
  
  5*10^-3 mol
- D.
  
  3.99 *10^-3 mol
9.

A+B -------> C. if ( V=k[A]ⁿ* [B]^m ) and [A]=0.1 ,[B]=0.5 ,,, find V and K ? [A] [B] V 0.25 0.25 0.2130 0.25 0.125 0.1065 0.2 0.1 0.0682 0.35 0.1 0.1193 0.175 0.1 0.0596
- A.
  
  V=0.1705 M/S K=3.41 M^-1.S^-1
- B.
  
  V= 0.77 M/S K = 3.3 M
- C.
  
  V= 1.3 M/S K = 4.1 M^-2.S^-2
- D.
  
  V=1.1 M/S K=0.5 S^-1
10.

A catalyst:
- A.
  
  Increase reaction rate by lowering the activation energy of forward reaction
- B.
  
  Increase reaction rate by increasing activation energy for reverse reaction
- C.
  
  Increase the reaction rate by providing an alternative energy
- D.
  
  None of the above
11.

(2NO+Br^-2 ----------> 2NOBr) KC₁=2 ( 2NO^- -------> N₂+O₂) KC₂=2.1*10³⁰ At temperature=298 K Calculate Kp of (N₂+O₂+Br^-2à2NOBr)
- A.
  
  4.2*10³⁰
- B.
  
  9.5*10^-31
- C.
  
  3.9*10^-32
- D.
  
  4*10^-32
12.

Calculate pH for .5 M of HF (Ka =7.1*10^-4)
- A.
  
  1.725
- B.
  
  0.01884
- C.
  
  3.77
- D.
  
  4.4
13.

A substance that is capable of acting as both acid and base is called:
- A.
  
  Conjugated
- B.
  
  Amphoteric
- C.
  
  Autocratic
- D.
  
  None
14.

Mixture of 5 ml of .105 M KOH and 15 ml of 9.5*10^-2 M of Ca(OH)₂ find Ph ?
- A.
  
  0.1425
- B.
  
  0.77
- C.
  
  0.16875
- D.
  
  13.23
15.

Which of the following correctly relates the two equilibrium constant for two reaction shown. .. (NOCl-------->NO +1/2 Cl₂) K1. (2No+Cl₂ -------> 2Nocl ) K2
- A.
  
  K₂=K₁
- B.
  
  K₂₌1/(K₁)²
- C.
  
  K₂=K₁
- D.
  
  None
16.

Which of the following compounds doesn’t show buffer:
- A.
  
  NH₃ / NH⁺⁴
- B.
  
  HCO^-3 / H₂CO₃
- C.
  
  NaOH / OH^-
- D.
  
  None
17.

At freezing point of water 0c⁰ when Kw = 1.2*10^-15 , calculate [H⁺] and [OH^-] for natural solution:
- A.
  
  1.2*10^-15
- B.
  
  3.46*10^-8
- C.
  
  2.6*10^-7
- D.
  
  None
18.

Calculate PH if [OH] = 1.9*10 ^-6
- A.
  
  5.72
- B.
  
  8.28
- C.
  
  5.26
- D.
  
  None
19.

Calculate Ka of NH₄⁺(Kb of NH₃= 1.8*10^-5)
- A.
  
  10^-4
- B.
  
  5.6*10^-10
- C.
  
  1.8*10^-7
- D.
  
  2*10^-3
20.

The mixture formed by adding 10 ml of .1 M HBr with 20 ml of .2 M HCl , calculate PH :
- A.
  
  0.1666
- B.
  
  0.778
- C.
  
  0.13
- D.
  
  0.114
21.

Classify each salt into (acidic, basic, natural) respectively: ( Nacl , CH₃NH₃Br , CH₃COONa )
- A.
  
  Natural, acidic, basic
- B.
  
  Acidic, basic, natural
- C.
  
  Natural, basic, acidic
- D.
  
  None
22.

How many moles of NH₄Cl must be added to 2 L of .1 M NH₃to form a buffer solution of PH=9 (Kb NH₃= 1.8*10^-5)?
- A.
  
  9.25
- B.
  
  0.18
- C.
  
  0.36
- D.
  
  0.22
23.

Calculate PH of .3 M NH₃ and .36 NH₄Cl , what is PH after adding 80 ml of buffer solution P_Ka= 9.25 (respectively)
- A.
  
  9.17 / 9.20
- B.
  
  9.20 / 9.17
- C.
  
  2.70 / 2.9
- D.
  
  None
24.

We have the following equilibrium (2SO₃ -------> 2SO₂+ O₂ ) what will happen to [SO₃] if the temperature is increased:
- A.
  
  Increase
- B.
  
  Decrease
- C.
  
  Not change
- D.
  
  Cannot tell
25.

PCl₅ ---> PCl₃+ Cl₂ if Kc =.497 if the initial concentration of PCl₅ = 1.66, calculate equilibrium concentration for (PCl5 / PCl₃/ Cl₂₎ (respectively):
- A.
  
  0.96 / 0.69 / 0.69
- B.
  
  0.69 / 0.69 /0 .69
- C.
  
  0.69 / 0.97 /0 .97
- D.
  
  None