Home
Class 12
CHEMISTRY
An athlete is given 100 g of glucose (C6...

An athlete is given 100 g of glucose (`C_6H_12O_6`) of energy equivalent to 1560 kJ. He utilises 50% of this gained energy in the event. In order to avoid the storage of energy in the body, calculate the weight of water he would need to perspire. The enthalpy of evaporation of water is `44 kJ mol^(-1)`.

Text Solution

Verified by Experts

`therefore` Energy Gained by the athelete `=(1560 xx 50/100) = 780` kJ
`therefore` Amount of water evaporated `=(780/44 xx 18)g = 319.14` gm
Promotional Banner

Similar Questions

Explore conceptually related problems

An athelete is given 100g of glucose (C_(6)H_(12)O_(6)) of energy equivalent to 1560 kJ . He utilises 50% of this gained enegry in the event. In order to avoid storage of enegry in the body, calculate the weight of water he would need to perspire. The enthalpy of evaporation of water is 441kJ//mol .

An athlete is given 180 g of glucose (C_(6)H_(12)O_(6)) . He utilises 50% of the energy due to internal combustion in the body. In order to avoid storage of energy in the body, calculate the masss of water he would need to perspire. Given enthalpy of combustion of glucose is -2800 kJ mol^(-1) and enthalpy of evaporation of water is 44 kJ mol^(-1)

An athlete is given 180 g of glucose (C_(6)H_(12)O_(6)) . He utilises 50% of the energy due to internal combustion in the body. In order to avoid storage of energy in the body, calculate the masss of water he would need to perspire. Given enthalpy of combustion of glucose is -2800 kJ mol^(-1) and enthalpy of evaporation of water is 44 kJ mol^(-1)

An athlete takes 100 g of glucose of energy equivalent to 1560 kJ. How much amount of energy is uptaken by 1 g molecule of glucose?

Calculate the entropy change when 3.6g of liquid water is completely converted into vapour at 100^(@)C . The molar heat of vaporization is 40.85KJ mol^(-1) .

18g of water is taken to prepare the tea. Find out the internal energy of vaporisation at 100^(@) C. (Delta_(vap)H for water at 373 K is 40.66kJ mol^(-1))

A swimmer coming out from a pool is covered with a film of water weighing about 80g . How much heat must be supplied to evaporate this water ? If latent heat of evaporation for H_(2)O is 40.79 kJ mol^(-1) at 100^(@)C .

A swimmer coming out from a pool is covered with a film of water weighing about 80g . How much heat must be supplied to evaporate this water ? If latent heat of evaporation for H_(2)O is 40.79 kJ mol^(-1) at 100^(@)C .

90 g of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at 100^(@)C . (Given the molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^(-1) ).

90 g of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at 100^(@)C . (Given the molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^(-1) ).