Q. With rise in pressure, the solubility of gases in solvent, at a fixed temperature

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Q. Pick out the wrong statement.

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Q. Vapor pressure of water at 100°C is about __________ bar.

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Q. At room temperature, the product [H⁺] [OH⁻] in a solution is 10⁻¹⁴ moles/litre. If, [OH⁻] = 10⁻⁶ moles/litre, then the pH of the solution will be

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Q. Molar heat capacity of water in equilibrium with ice at constant pressure is

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Q. If pH value of a solution is 8, then its pOH value will be

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Q. The chemical nature of an element is independent of

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Q. The heat change for the reaction, C(s) + 2S(s) → CS₂(l), is 104.2 kJ. It represents the heat of

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Q. A sample of well water contains 140 gm/m³ Ca²⁺ ions and 345 gm/m³ Na⁺ ions. The hardness of the sample of water, expressed in terms of equivalent CaCO₃ in gm/m³ is (assuming atomic masses of Ca :40, Na : 23, C : 12, O : 16)

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Q. The activity co-efficient of a solution, which accounts for the departure of liquid phase from ideal solution behaviour

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Q. Osmotic pressure of a dilute solution of a non volatile solute in a solvent obeying Raoult's law is proportional to the

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Q. In case of an unsaturated vapor-gas mixture, the humid volume increases with increase in the

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Q. Which of the following is an exothermic reaction ?

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Q. Heat of solution in a system in which both solute and solvent are liquids is termed as

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Q. A solution is made by dissolving 1 kilo mole of solute in 2000 kg of solvent. The molality of the solution is

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Q. Average molecular weight of air is about

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Q. 6 gms of magnesium (atomic weight = 24), reacts with excess of an acid, the amount of H₂ produced will be __________ gm.

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Q. Pick out the wrong unit conversion of calorific value.

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Q. Increasing the temperature of an aqueous solution will cause decrease in its

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Q. Assuming that CO₂ obeys perfect gas law, calculate the density of CO₂ (in kg/m³) at 263°C and 2 atm.

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