DAILY TEST 2
CHEMISTRY
CLASS XI
Fill in the blank
1.
The ionization reaction of Fe2 (SO4)3 is…..
2.
Write down two the example of homogenous
equilibria reaction
3.
Write down two the example of heterogenous
equilibria reaction
4.
Write down the effect of temperature to the
shift of an equailibrium
5.
Write down the effect of concentration to the
shift of an equailibrium
6.
Write down the effect of pressure and volume the
shift of an equailibrium
7.
Write down the effect of catalyst to the shift
of an equailibrium
8.
Write down one example of an equilibrium
reaction and also its formula
equilibrium constant.
9.
If
several reaction are added , the value of equilibrium constant from
addition of the reactions is ………
10.
If a reaction
is reversed, the value of equilibrium constant of the inverse reaction
is………
11.
If a
reaction is multiplied by the number of n, the value of the equilibrium
constant becomes…..
12.
If a reaction is devided by the number of n, the
value of the equilibrium constant becomes …..
13.
According to Arrhenius acid is……
14.
According to
Arhenius base is….
15.
Write down 5 compounds belong to acid
16.
Write down the 5 compound belong to base
17.
Calculate
the pH of HCl 0.01 M
18.
Calculate the pH of HNO2 0.05 M , if
the value of Ka for acid is 5 x 10-4
19.
Calculate the pH of Ba(OH)2 0.1 M
20.
According to Bronsted-Lowry acid is…
21.
According to Bronsted- Lowry base is…..
22.
What is conjugate acid ? and show it with reaction
23.
What is conjugate base? And show it with a
reaction
24.
A reaction proceeds according to the equation of
X à Y. Initially,
concentration of X is 0.6 M , after 10 seconds
it becomes 0.2 M , the reaction rate is…………
25.
According to Lewis acid is…
26.
According to Lewis base is….
27.
Reaction rate is…………
28.
The unit of reaction rate is…………
29.
Reaction order is…………
30.
If the concentration of substance X is increased
to two times, actually the reaction rate of the substance increases to 8 times.
Calculate the reaction rate to the substance X.
Essay Test
1.
In the dissociation reaction of N2O4
gas into NO2 gas the equilibrium state occurs represented by
reaction equation as follows.
N2O4(g) ↔ 2NO2(g)
If
the concentration of N2O4 and NO2 is
1.71 M and 0.58 respectively, calculate the value of Kc at that
state. (( 0,2 )
2.
If 0.6
moles of HI gas id filled into a container of 1 liter at temperature of 4580C,
the mixture in an equilibrium id found to contain of 0.066 moles of I2
gas, calculate tha value of Kc for the equilibrium reaction of 2HI(g)
↔
H2 (g) + I2(g) at that temperature.
3.
As much as 0.2 moles of HI is filled into a container
of 1 liter ,so an equilibrium occurs according to the following equation. 2HI(g) ↔ H2
(g) + I2(g)
If the dissociation degree of HI gas is known to be
equal to 0.25 ,calculate the value of Kc.
4.
Given that reaction as follows.
N2 + O2 ↔ 2NO Kc1 = 4 x 10-3
N2 + ½ O2 ↔
N2O Kc2
= 2,5 x 10-2
Calculate the Kc for the
reaction of : N2O + ½O2 ↔
2NO
5.
A substance X reacts to Y based on this chemical
equation.
X à
Y . If the initial concentration of Y = 0.5 M and after reacting to X during
one minute, the concentration becomes 0.2 M . Determine the reaction rate with
respect to Y.
6.
If at a certain temperature the rate of N2O5
disscociation in to NO2 and O2 is 2.5 x 10-6
mol/L second, calculate the rate of O2 formation.
7.
If at a certain temperature the rate of N2O5
disscociation in to NO2 and O2 is 2.5 x 10-6
mol/L second, calculate the rate of NO2 formation.
8.
An experiment conducted to observe a reaction of
: 2NO + 2H2 à 2H2O
|
No
|
[NO] M
|
[H2] M
|
V
(M/s)
|
|
1
|
0.1
|
0.1
|
2
|
|
2
|
0.1
|
0.2
|
32
|
|
3
|
0.4
|
0.1
|
64
|
Determine :
a.
Reaction order
b.
The reaction rate equation
c.
Reaction rate constant ( K)
9.
The experiment data of the reaction 2A + B2 à
2AB are as follows .
|
No
|
[A] M
|
[B2] M
|
V
(M/s)
|
|
1
|
0.5
|
0.5
|
1.6 x 10-4
|
|
2
|
0.5
|
1
|
3.2 x 10-4
|
|
3
|
1
|
1
|
3.2 x 10-4
|
Determine :
a.
Reaction orders
b.
Reaction rate equation
c.
Reaction rate constant (k)
d.
The reaction rate of the concentration of A is 0.1 and B2 is 0.2
10.
Explain 5 factors that influence reaction rate.
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