Chemistry 102 : Can You Pass This Trivia Test? Quiz
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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!
- 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*10-3 m
- B.
9.175*10-4 m
- C.
8.1*10-4 m
- D.
9.9*10-4 m
- 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*10-3 mol
- 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 NH3 to 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 PKa = 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
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