100 g of water is supercooled to `-10^@C` . At this point, due to some disturbance mechanised or otherwise some of its suddenly freeazes to ice What will be the temperature of the resultant mixture and how much mass would freeze?
`(S_W = 1 cal//g//^@C` and `L_(W fusion)` = 80 cal/g].

Assuming a domestic refrigerator a reversible engine working between melting point of ice and the room temperature of 17^@C .Calculate the enrgy in joule that m ust be suppled to freeze 2kg of water .Given that temperature of water = 0^@C nd L=80 cal//g .

1 g of water cools down from its boiling point to its freezing point, it gives off about 420 J of heat energy. By how much does its mass change because of this loss in energy?

18 g of a compound is dissolved in 10 kg of water so that the resulting solution freezes at - 8^(@) C . If K_(f) for water = 1 . 86 K/m . Calculate the molecular mass of the compound

Gasoline has an enthalpy of combustion 24000 kJ/mol gallon. When gasoline burns in an automobile engine, approximately 30% of the energy released is used to produce mechanical work. The remainder is lost as heat transfer to the engine's cooling system. As a start on estimating how much heat transfer is required, calculate what mass of water could be heated from 25^(@)C to 75^(@)C by the combustion of 1.0 gallon of gasoline in an automobile? (Given : C(H_(2)O)=4.18 J//g^(@)C ) a) 34.45 kg b) 80.383 kg c) 22 kg d) 224 kg

1 . 5 of Ba (NO_(3))_(2) dissolved in 100 g of water shows a depression in freezing point equal to 0 . 28^(@)C . What is the percentage dissociation of the salt ? ( K_(f) for water = 1 . 86 K/m and molar mass of Ba (NO_(3))_(2) = 261.)

10g of non-volatile solute when dissolved in 100g of benzene raises its boiling point by 1^@ C. What is the molecular mass of the solute. ( k_b for benzene=2.53 K kg mol^-1 )

35 g of compound is added in 1 kg of water so that the resulting solution freezes at - 10^(@) C . If K_(f) for water = 1. 86 K/m . Calculate the molecular mass of the compound

A mixture of H_(2)SO_(4) and H_(2)C_(2)O_(4) (oxalic acid ) and some inert impurity weighing 3.185 g was dessolved in water and the solution made up to 1litre. 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another experiment 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO_(4) solution for complete reaction. The mass % of H_(2)SO_(4) in the mixture was: