A sample of 16 g charcoal was brought into contact with `CH_(4)` gas contained in a vessel of 1 litre at `27^(@) C` . The presses of gas was found to fall from 760 to 608 torr. The density of chacoal sample is `1.6 g//m^(3)` . What is the volume of the `CH_(4)` gas adsorbed per gram of the adsorbent at 608 torr and `27^(@)C`?
At 273°C and 380 torr pressure, the density of a gas is 1.25 kg//^(3) . So its density at STP in g// is
A sample of CH_(4) of 0.08g was subjected to combustion at 27^(@)C in a bomb calorimeter. The temperature of the calorimeter system was found to be raised by 0.25^(@)C . If heat capacity of calorimeter is 18 kJ//""^(@)C, Delta H for combustion of CH_(4) at 27^(@)C is
A flask contains 1gm, of H_2 , 2gms. of Ne and 1.6 gms. of O_2 at a pressure of 2 atmoshperes at 27^@C . Calculate the partial pressures of each gas and the volume of the flask.
One mole of carbon-dioxide was found to occupy a volume of 1.32 litre at 48^(@) C and at a pressure of 16.4 atm. Calculate the pressure of the gas that would have been expected to behave ideally and non-ideally.
Density of a gas is found to be 5.46g/dm^3 at 27^@C at 2 bar pressure. What will be its density of STP?
Find the volume of 8g of oxygen gas at 27^@C and 1 atmosphere prressure. If the volume of each molecule is 3.4 xx 10^(-24)c c calculate the vacant space in the gas.
NARENDRA AWASTHI-SURFACE CHEMISTRY-Level 3 - Assertion - Reason Type Questions
