The hydrogen electrode is dipped in a solution of pH = 3 at 25°C. The potential of the cell would be [use value of = 0.59 V]
0.059 V
0.088 V
0.178 V
-0.177 V
D.
-0.177 V
Since, reduction potential for hydrogen electrode is
EH =
Given pH = 31; e - log = 3
EH = -0.059 × pH = -0.059 × 3
= -0.177 V
Reaction between compounds (A) and (B) occurs as follows
A (g) + 2B (g) → 2C (g)
Following results were obtained
(1) Exp. No. | (2) Initial concentration of [A] mol L-1 | (3) Initial concentration of [B] mol L-1 | (4) Initial rate of formation of [C] mol L-1 s-1 |
1. | 0.30 | 0.30 | 0.10 |
2. | 0.30 | 0.60 | 0.40 |
3. | 0.60 | 0.30 | 0.20 |
The correct rate- law for the said reaction is (r and k rate and rate constant respectively)
r = k[A]2B
r = k[A][B]2
r = k[A][B]
r = k[A]2[B]2
In the reaction 2NO2 N2O4; the rate of disappearance of NO2 is equal to
2 [NO2]2
2k1[NO2]2 - 2k2[N2O4]
2k2[NO2]2 - k2[N2O4]
(2k1 - k2)[NO2]
The rate constant for the raection 2N2O5 → 4NO2 + O2 is 3.0 × 10-5 s-1. If rate is 2.40 × 10-5, then concentration of N2O5 (in mol/L) is
1.4
1.2
0.04
0.8
In the reaction,
CH3-CH2-Cl (A) (B), end product (B) is
CH3 - CH2 - CN
CH3 - CH2 - CONH2
CH3 - CH2 - COOH
CH3 - CH2 - CH2 - CH2 - CN
On Friedal Crafts acetylation, anisol yields
2-methoxyacetophenone
4-methoxyacetophenone
Both (a) and (b)
None of the above