Which one of the following orders correctly represents the increasing acid strengths of the given acids?
1.
2.
3.
4.
For the reaction,
CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
ΔrH = -170.8 kJ mol-1
Which of the following statements is not true?
1. | At equilibrium, the concentration of \(\mathrm{CO}_2 \mathrm{~g}\) and water (l) are not equal. |
2. | The equilibrium constant for the reaction is given by \(K_p=\frac{\left[\mathrm{CO}_2\right]}{\left[\mathrm{CH}_4\right]\left[\mathrm{O}_2\right]}\) |
3. | The addition of \(\mathrm{CH}_4 \mathrm{~g} \) or \(\mathrm{O}_2 \mathrm{~g}\) at equilibrium will cause a shift to the right |
4. | The reaction is exothermic |
The following pair constitutes a buffer is:
1.
2.
3.
4.
The hydrogen ion concentration of a 10-8 M HCl aqueous solution at 298 K (Kw = 10-14) is:
1.
2.
3.
4.
The ionic species that has the greatest proton affinity to form stable compound is:
1.
2.
3.
4.
The following equilibrium constants are given:
N2 + 3H2 ⇌ 2NH3; K1
N2 + O2 ⇌ 2NO; K2
H2 + 1/2O2 ⇌ H2O; K3
The equilibrium constant for the oxidation of NH3 by oxygen to give NO is:
1.
2.
3.
4.
A weak acid, HA, has a Ka of 1.00×10-5. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to:
1. 99.0%
2. 1%
3. 99.9%
4. 0.100%
The pOH of a solution at 25 °C that contains 1×10-10 M of hydronium ions is:
1. | 7.00 | 2. | 4.00 |
3. | 9.00 | 4. | 1.00 |
The value of the equilibrium constant of the reaction
is 8.0.
The equilibrium constant of the reaction
will be-
1. | \(1 \over 16\) | 2. | \(1 \over 64\) |
3. | 16 | 4. | \(1 \over 8\) |
The value of KP1 and Kp2 for the reactions
are in the ratio of 9 : 1. If the degree of dissociation of X and A is equal, then the total pressure at equilibrium(i) and (ii) are in the ratio:
1. 3 : 1
2. 1 : 9
3. 36 : 1
4. 1 : 1