Single Choice

An aqueous solution of methanol in water has vapour pressure:

Aequal to that of water
Bequal to that of methanol
Cmore than that of water
Correct Answer
Dless than that of water

Solution

The vapour pressure of an aqueous methanol solution is more than that of water but less than that of methanol. This is due to solute-solvent interaction is more due to the formation of hydrogen bonding than methanol but less than water.

The hydrogen of $$CH_3OH$$ (methanol) and oxygen of $$H_2O$$ (water) form a hydrogen bond and vice-versa.

SIMILAR QUESTIONS

Solutions

The pressure at which liquid and vapour can coexist at equilibrium is called the :

Solutions

The vapour pressures of two liquids A and B in their pure states are in the ratio of 1 : 2. A binary solution of A and B contains A and B in the mole proportion of 1 : 2. The mole fraction of A in the vapour phase of the solution will be:

Solutions

Calculate the vapour pressure of an aqueous solution of 1.0 molal glucose solution at $$100^oC.$$

Solutions

Two moles of $$O_2$$ gas is collected over water at 400 K temperature in 2 litre vessel. If the pressure of dry $$O_2$$ gas is 32.20 bar then find the vapour pressure of water under the same conditions.

Solutions

Two moles of pure liquid 'A' $$(P_{A}^{0} =80mm$$ of Hg) and $$3$$ moles of pure liquid 'B' ($$P_{B}^{0} = 120mm$$ of Hg) are mixed. Assuming ideal behaviour?

Solutions

The vapour pressure of a solvent at $$293$$K is $$100$$ mm Hg. Then the vapour pressure of a solution containing $$1$$ mole of a strong electrolyte $$(AB_2)$$ in $$99$$ moles of the solvent at $$293$$ K is: (Assume complete dissociation of solute)

Solutions

A zinc metal sample containing zinc chloride as impurity was made to react with an excess of dilute hydrochloric acid at $$ 27^{o}C$$. Liberated hydrogen gas is collected at 760 mm Hg pressure that occupies $$780.0 cm^{3}$$ volume. If the vapour pressure of water at $$27^{o}C$$ is 14 mm Hg, what is the volume of $$H_{2}$$ at STP? The Standard pressure is 760 mm Hg (molar volume of gas at standard temperature and pressure, $$STP = 22.4 dm^{3}$$)

Solutions

Liquid $$M$$ and liquid $$N$$ form an ideal solution. The vapour pressures of pure liquids $$M$$ and $$N$$ are $$450$$ and $$700\ mm$$ $$Hg$$, respectively, at the same temperature. Then correct statement is: ($${x}_{M}=$$ Mole fraction of $$M$$ in solution; $${x}_{N}=$$ Mole fraction of $$N$$ in solution; $${y}_{M}=$$ Mole fraction of $$M$$ in vapour phase; $${y}_{N}=$$ Mole fraction of $$N$$ in vapour phase)

Solutions

In three beakers labeled as (A), (B) and (C), $$100mL$$ of water, $$100mL$$ of $$1M$$ solution of glucose in water and $$100mL$$ of $$0.5M$$ solution of glucose in water are taken respectively and kept at same temperature. Which of the following statements is correct?

Solutions

The given graph shows the vapour pressure temperature curves for some liquids.Liquids A,B,C and D respectively are :

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