For the reaction N2 (g) + O2 (g) ⇌ 2NO (g), the equilibrium constant is K1. The equilibrium constant is K2 for the reaction 2NO (g) + O2(g) ⇌ 2NO2 (g). What is K for the reaction 
1/(4K1K2)
[1/K1K2]1/2
1/(K1K2)
1/(K1K2)
B.
[1/K1K2]1/2
N2 (g) + O2 (g) ⇌ 2NO (g) ; K1 (i)
2NO (g) + O2 (g) ⇌ 2NO2 (g) ; K2 (ii)
______________________________
N2 (g) + O2(g) ⇌ 2NO2 (g) ; K = K1 x K2
therefore, For NO2 (g) = N2/2 (g) +O2 (g);
K = [1/K1K2]1/2
The value of ΔH for the reaction
X2 (g) + 4Y2 (g) ⇌ 2XY4 (g) is less than zero. Formation of XY4 (g) will be favoured at
Low pressure and low temperature
high temperature and low pressure
high pressure and low temperature
high pressure and low temperature
C.
high pressure and low temperature
X2 (g) + 4Y2 (g) ⇌ 2XY4 (g);
Which one of the following pairs of the solution is not an acidic buffer?
HClO4 and NaClO4
CH3COOH and CH3COONa
H2CO3 and Na2PO4
H2CO3 and Na2PO4
A.
HClO4 and NaClO4
A buffer solution is one which resists changes in pH when small quantities of an acid or an alkali are added to it.
HClO4 and NaClO4 are not an acidic buffer because strong acid with its salt cannot form buffer solution.A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH4 is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 x 10-5, what is the pH of this solution?
log ( 2.7 = 0.43)
9.43
11.72
8.73
9.08
A.
9.43
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
12.65
2.0
7.0
7.0
A.
12.65
When equal volumes of acid and base are mixed then resulting solution become alkaline if the concentration of base is taken high.
Let normality of the solution after mixing 0.1 M
NaOH and 0.01 M HCl is N.
therefore, N1V1 - N2V2 = NV
or 0.1 x 1 - 0.01 x 1 = N x 2
Since normality, of NaOH, is more than that of HCl. Hence, the resulting solution is alkaline.
Or
[OH-] = N = 0.09/2 = 0.045 N
Or pOH = - log (0.045) = 1.35
therefore, pH = 14-pOH
= 14 - 1.35 = 12.65
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