An ideal gas expands in volume from 1$$\times$$10-3 m3 to 1 $$\times$$ 10-2 m3 at 300 K against a constant pressure of 1$$\times$$105 Nm-2. The work done is :

The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283 kJ mol-1 respectively. The enthalpy of formation of carbon monoxide per mole is :

On mixing ethyl acetate with aqueous sodium chloride, the composition of the resultant solution is

Which of the following undergoes reaction with 50% sodium hydroxide solution to give the corresponding alcohol and acid?

Which one of the following reduced with zinc and hydrochloric acid to give the corresponding hydrocarbon?

6.02 $$\times$$ 1020 molecules of urea are present in 100 ml of its solution. The concentration of urea solution is (Avogadro constant, NA = 6.02 $$\times$$ 1023 mol-1)

To neutralise completely 20 mL of 0.1 M aqueous solution of phosphorous acid (H3PO3), the volume of 0.1 M aqueous KOH solution required is

The ammonia evolved from the treatment of 0.30 g of an organic compound for the estimation of nitrogen was passed in 100 mL of 0.1 M sulphuric acid. The excess of acid required 20 mL of 0.5 M sodium hydroxide solution for complete neutralization. The organic compound is

Which one of the following ores is best concentrated by froth – floatation method?

For which of the following parameters the structural isomers C2H5OH and CH3OCH3 would be expected to have the same values? (Assume ideal behaviour)

Which of the following liquid pairs shows a positive deviation from Raoult’s law?

Which one of the following aqueous solutions will exhibit highest boiling point?

Which one of the following statements is false?

What is the equilibrium expression for the reaction P4 (s) + 5O2 $$\leftrightharpoons$$ P4O10 (s)?

For the reaction, CO(g) + Cl2(g) $$\leftrightharpoons$$ COCl2(g) the {{{K_p}} \over {{K_c}}} is equal to :

The equilibrium constant for the reaction N2(g) + O2(g) $$\leftrightharpoons$$ 2NO(g) at temperature T is 4 $$\times$$ 10-4. The value of Kc for the reaction NO(g) $$\leftrightharpoons$$ 1 \over 2N2 (g) + 1 \over 2O2 (g) at the same temperature is :

The smog is essentially caused by the presence of :

In a hydrogen – oxygen fuel cell, combustion of hydrogen occurs to :

Consider the following Eo values $$E_{F{e}^{3+}/F{e}^{2+}}^o$$ = 0.77 V; $$E_{S{n}^{2+}/Sn}^o$$ = -0.14 V Under standard conditions the potential for the reaction Sn(s) + 2Fe3+(aq) $$\to$$ 2Fe2+(aq) + Sn2+(aq) is :

The standard e.m.f of a cell, involving one electron change is found to be 0.591 V at 25oC. The equilibrium constant of the reaction is (F = 96,500 C mol-1: R = 8.314 JK-1 mol-1)