A ideal gas does work on its surroundings when it expands by 2.5 L against external pressure 2 atm. This work done is used to heat up 1 mole of water at 293 K. What would be the final temperature of water in kelvin if specific heat for water is "4.184 Jg"^(-1)"K"^(-1)?

A ideal gas does work on its surroundings when it expands by 2.5 L aga

1.	A ideal gas does work on its surroundings when it expands by 2.5 L against external pressure 2 atm. This work done is used to heat up 1 mole of water at 293 K. What would be the final temperature of water in kelvin if specific heat for water is "4.184 Jg"^(-1)"K"^(-1)?
Answer» 300 600 200 1000 Solution :WORK DONE, `w=-P_("ext.")DV` `W=-2xx2.5=-"5 L atm"=-"506.3 J"` Because this work is used in raising the temperature of water, so work done is equalto the HEAT supplied i.e., `w=q=m.c_(s).DeltaT` Given that, `m= 18g"(= 1 mole)", c_(s)=4.184g^(-1)K^(-1)`, `q=+506.3J, DeltaT=? `(Heat is given to water) `DeltaT=(q)/(c_(s).m)=(506.3)/(4.184xx18)=6.72` `therefore"FINAL temperature, "T_(f)=T_(i)+DeltaT=293+6.72` `=299.72K~~300K`