H_(2)S , a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of H_(2)S in water at STP is 0.195m, calculate Henry's law constant.
The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen at 298 K are 3.30 xx10^(7) mm and 6.51 xx10^(7) mm respectively, calculate the composition of these gases in water .
If water turns into ice. at a pressure of 1 atmosphere and 0^@ C then the temperature of this system during this process -
Vapour pressure of pure water at 298 K is 23.8 mm Hg. 50g urea (NH_(2)CONH_(2)) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and its relative lowering. Consider Raoult's law and formula for relative lowering in vapour pressure, (P_(A)^(0)-P_(s))/(P_(A)^(0))=(n_(B))/(n_(A))=(W_(B))/(M_(B))xx(M_(A))/(W_(A)) Where, (P_(A)^(0)-P_(s))/(P_(A)^(0)) is called relative lowering in vapour pressure.
O_2 is bubbled through water at 293K, assuming that O_2 exerts a partial pressure of 0.98 bar, the solubility of O_2 in gm. L^(-1) is (Henry's law constant = 34 k bar)
If N_(2) gas is bubbled through water at 293 K, how many millimoles of N_(2) gas would dissolve in 1 litre of water ? Assume that N_(2) exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N_(2) at 293 K is 76.48 k bar.
When 1 gm of water changes from liquid to vapour phase at constant pressures of 1 atmosphere, the volume increases from 1 cc to 1671 cc. The heat of vaporisation at this pressure is 540 cal/gm. Increase in internal in internal energy of water is (1 atmosphere = 1.01xx10^(6) "dyne/cm"^(2))
If 0.05 mole of gas are dissolved in 500 grams of water under 1 atm. pressure, 0.1 moles will be dissolved if the pressure is 2atm. It illustrates
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
