States of Matte...

Equal masses of $$SO_2, CH_4$$ and $$O_2$$ are mixed in empty container at $$298$$K, where total pressure is $$2.1$$ atm. The partial pressures of $$CH_4$$ in the mixture is:

The vapour pressure of a pure liquid A is $$70$$ torr at $$27^o$$C. It forms an ideal solution with another liquid B. The mole fraction of B is $$0.2$$ and total vapour pressure of the solution is $$84$$ torr at $$27^o$$C. The vapour pressure of pure liquid B at $$27^o$$C.

If 2 moles of A and 3 moles of B are mixed to form an ideal solution vapour pressure of A and B are 120 and 180 mm of Hg respectively. then the composition of A and B in the Vapour phase when the first traces of vapour are formed in the above case is:

The mass of $$350{ cm }^{ 3 }$$ of a diatomic gas at 273 K at 2 atmospheres pressure is one gram. Calculate the mass of one atom of the gas.

Starting with one mole of nitrogen and 3 moles of hydrogen, at equilibrium $$50\%$$ of each had reacted according to the reaction: $$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$$
If the equilibrium pressure is $$P$$, the partial pressure of hydrogen at equilibrium would be:

The Total pressure in a mixture of $$8g$$ of dioxygen and $$4g$$ of dihydrogen confined in a vessel of $$1dm^34$$ at $$27^oC$$ is ?

Calculate the volume occupied by 16 gram $$O_2$$ at 300K and 8.31 MPa if $$\dfrac{P_cV_c}{RT_c}$$ = 3/8 and $$\dfrac{P_rV_r}{T_r}$$=2.21.
(Given : R = 8.314 J/ K-mol)

A Solution of non-volatile solute in water freezes at $$-0.{ 30 }^{ }C.$$ The vapour-pressure of pure water at $$298K$$ is $$23.51mm Hg$$ and $${ K }_{ 1 }$$ for water is $$1.86 K. kg { mol }^{ -1 }$$ Calculate the vapour-pressure of this solution at $$298K.$$

In the following graphical representation for reaction $$A \to B$$ there are two types of regions:

Which of the following gases has the highest density under standard conditions?