States of Matte...

The density of a liquid is 1.2 g/mL. That are 35 drops in 2 mL. The number of molecules in 1 drop is (molecular weight of liquid = 70): 

The reaction, $$ZnO(s)+CO(g) \rightleftharpoons  Zn(g)+{CO}_{2}(g)$$, has an equilibrium constant of $$1$$ atm at $$1500K$$. The equilibrium partial pressure of zinc vapour in a reaction vessel if an equimolar mixture of $$CO$$ and $${CO}_{2}$$ is brought into contact with solid $$ZnO$$ at $$1500K$$ and the equilibrium is achieved at $$1$$ atm is?

When a liquid that is immiscible with water was steam distilled at $$95.2^o$$C at a total pressure of $$99.652$$ kPa, the distillate contained $$1.27$$ g of the liquid per gram of water. What will be the molar mass of the liquid if the vapour pressure of water is $$85.140$$ kPa at $$95.2^o$$C?

If one mole monoatomic ideal gas was taken through process $$AB$$ as shown in figure, then select correct option(s).

An ideal gas undergoes isothermal expansion from ($$10$$ atm, $$1$$L) to ($$1$$ atm, $$10$$L) either by path-I(infinite stage expansion) or by path-II(first against $$5$$atm and then against $$1$$ atm). The value of $$\left(\displaystyle\frac{q_{path-1}}{q_{path-II}}\right)$$ is?

In which of the following case(s) pressure of gas is more than atmospheric pressure.

$$18$$ g glucose ($$C_6H_{12}O_6$$) is added to $$178.2$$ g of water. The vapour pressure of this aqueous solution at $$100^0C$$ in torr is:

Two liquids $$X$$ and $$Y$$ from an ideal solution. At $$300K$$, a vapour pressure of the solution containing $$1$$ mol of $$X$$ and $$3$$ mol of $$Y$$ is $$550$$ $$mm \ Hg$$. At the same temperature, if $$1$$ mol of $$Y$$ is further added to this solution, a vapour pressure of the solution increased by $$10$$ $$mm \ Hg$$. Vapour pressure ( in mmHg) of $$X$$ and $$Y$$ in their pure states will be respectively: 

At certain temperature ($$T$$) for the gas phase reaction
$$2{ H }_{ 2 }O(g)+2{ Cl }_{ 2 }(g)\rightleftharpoons 4HCl(g)+{ O }_{ 2 }(g);{ K }_{ P }=12\times { 10 }^{ 8 }atm$$
If $${Cl}_{2}$$, $$HCl$$ and $${O}_{2}$$ are mixed in such a manner that the partial pressure of each is $$2atm$$ and the mixture is brough into contact with excess of liquid water. What would be approximate partial pressure of $${Cl}_{2}$$ when equilibrium is attained at temperature ($$T$$)?
[Given:Vapour pressure of water is $$380mm$$ $$Hg$$ at temperature ($$T$$)]

$$CuSO_4$$$$\cdot$$$$5H_2O(s)$$$$\rightleftharpoons$$ $$CuSO_4\cdot$$ 3$$H_2O(s)$$ + $$2H_2O(g)$$; $$K_p$$ = 4$$\times10^{-4}$$ $$atm^2$$ if the vapour pressure of water is 38 torr then percentage of relative humidity is: ( Assume all data at constant temperature)