Equilibrium Tes...

For the gas phase reaction : $$ 2NO(g) \leftrightharpoons N_2(g) +O_2 (g) ; \Delta H = -43.5 $$ kcal. Which one of the following is true for the reaction: $$ N _2(g) + O_2(g) \leftrightharpoons 2NO(g) $$ ?

If $$ K_1$$ and $$K_2 $$ are the equilibrium constants for a reversible reaction at $$ T_1 K$$ and $$T_2 K $$ temperature, respectively $$ ( T_1 < T_2 ) $$ and the reaction takes place with neither heat evolution nor absorption, then

In a closed container following equilibrium will be attained:

n-caproic acid, $$C_{5}H_{11}COOH$$, found in coconut and palm oil is used in making artificial flavors, has solubility in water equal to $$11.6 g/L$$. The saturated solution has $$pH = 3.0$$. The $$K_{a }$$ of acid is

$$O_3$$ is prepared by subjecting $$O_2$$ to silent electric discharge. The favourable conditions for the formation of ozone according to Le-chatlier's principle are

A solution has initially $$0.1 M -HCOOH$$ and $$0.2 M- HCN$$. $$K_{a}$$ of $$HCOOH = 2.56 \times 10^{-4}$$, $$K_{a}$$ of $$HCN = 9.6 \times 10^{-10}$$. The only incorrect statement for the solution is $$(log 2 = 0.3)$$

Small amount of freshly precipitated magnesium hydroxides are stirred vigorously in a buffer solution containing $$0.25 M$$ of $$NH_{4}Cl$$ and $$0.05 M$$ of $$NH_{4}OH$$. $$[Mg^{2+}]$$ in the resulting solution is ($$K_{b}$$ for $$NH_{4}OH = 2.0 \times 10^{-5}$$ and $$K_{sp}$$ of $$Mg(OH)_{2} = 8.0 \times 10^{-12}$$)

In a system : $$ A(s) \leftrightharpoons 2B(g) +3C(g) $$ if the concentration of C at equilibrium is increased by a factor of 2, it will cause the equilibrium concentration of B to decrease by

The reaction : $$ MgCO_3(s) \leftrightharpoons MgO(s) + CO_2(g) $$ is in progress. if number of mole of MgO in the vessel is doubled at an instance?

The EMF of cell: $$ H_{2}(g)|$$ Buffer $$ \parallel $$ Normal calmelelectrod, is 0.70 V at $$ 25^{\circ}C,$$ when barometric pressure is 760 mm. What is the pH of the buffer solution? $$ E_{Calomel}^{0} = 0.28 V. [2.303 RTIF = 0.06]$$