Work done in expansion of an ideal gas from `4` litre to `6` litre against a constant external pressure of `2.1 atm` was used to heat up `1` mole of water at `293 K`. If specific heat of water is `4.2 J g^(-1)K^(-1)`, what is the final temperature of water?

Work done in expansion of an ideal gas from 4 litre to 6 litre against a constant external pressure of 2.5 atm was used to heat up 1 mole of water at 293K. If specific heat of water is 4.184Jg^-1K^-1 , what is the final temperature of water?

Work done in expansion of an idela gas from 4L to 6L against a constant external pressure of 2.5 atm was used to heat up 1mol of water at 293K . If specific heat of water is 4.184J g^(-1)K^(-1) , what is the final temperature of water.

Work done in expansion of an idela gas from 4L to 6L against a constant external pressure of 2.5 atm was used to heat up 1mol of water at 293K . If specific heat of water is 4.184J g^(-1)K^(-1) , what is the final temperature of water.

A gas expands from 10 litres to 20 litres against a constant external pressure of 10 atm. The pressure-volume work done by the system is

A gas expands from 10 litres to 20 litres against a constant external pressure of 10 atm. The pressure-volume work done by the system is

The amount of work done when a gas is expanded from a volume of 5 L to 10 L against a constant external pressure of 2 atm is used to heat 15 g of water present at a temperature of 300 K. Calculate the final temperature of water. (Given : molar heat capacity of water = 75.6 J. K^(-1). " mol"^(-1) ).