`54g` of aluminium is treated with `100mL` of `0.4M` `NaOH` solution. The volume of `H_(2)` gas evolved at `1atm` and `300K` is (assume that `H_(2)` behaves as an ideal gas and `R=0.082L.atm.mol^(-1).K^(-1)`, atomic mass of `Al=27`)

The volume strength (at STP) of 100 ml H_2O_2 solution which produce 5.6 litre of oxygen gas at 1 atm and 273K is :

2.8 g of a gas at 1atm and 273K occupies a volume of 2.24 litres. The gas can not be:

0.9 g Al reacts with dil. HCl to give H_(2) . The volume of H_(2) evolved at STP is (Atomic weight of Al = 27)

10mol of an ideal gas confined to a volume of 10L is released into atmosphere at 300K where the pressure is 1bar. The work done by the gas is (R = 0.083 L "bar" K^(-1)mol^(-1))

Calculate the work done when 2.5 mol of H_(2)O vaporizes at 1.0 atm and 25^(@)C . Assume the volume of liquid H_(2)O is negligible compared to that of vapour. Given 1 L atm =101.3 J and R = 0.082 L atm "mol"^(-1)K^(-1) .

If 100mL of 0.1M urea solution is mixed with 100mL of 0.2M glucose solution at 300K. Calculate osmotic pressure?

100mL of " 0.1 M NaOH" solution is titrated with 100mL of "0.5 M "H_(2)SO_(4) solution. The pH of the resulting solution is : ( For H_(2)SO_(4), K_(a1)=10^(-2))

The equilibrium constant for the reaction Br_2(l)+Cl_(2)(g)hArr2Br Cl(g) at 27^@C is k_P=1 atm in a closed container of volume 164 L initially 10 moles of Cl_2 are present at 27^@C . What minimum mole of Br_2(l) must be introduced into this container so that above equilibrium is maintained at total pressure of 2.25 atm.Vapour pressure of Br_2(l) at 27^@C is 0.25 atm.Assume that volume occupied by liquid is negligible . [R=0.082 L atm "mole"^(-1) K^(-1) , Atomic mass of bromine =80]

If 100mL of 0.1M urea solution is mixed with 300mL of 0.2M glucose solution at 300K. Calculate osmotic pressure?

If 100mL of 0.1M urea solution is mixed with 200mL of 0.2M glucose solution at 300K. Calculate osmotic pressure?