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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» <html><body><p>300<br/>600<br/>200<br/>1000</p>Solution :<a href="https://interviewquestions.tuteehub.com/tag/work-20377" style="font-weight:bold;" target="_blank" title="Click to know more about WORK">WORK</a> <a href="https://interviewquestions.tuteehub.com/tag/done-2591742" style="font-weight:bold;" target="_blank" title="Click to know more about DONE">DONE</a>, `w=-P_("ext.")<a href="https://interviewquestions.tuteehub.com/tag/dv-433533" style="font-weight:bold;" target="_blank" title="Click to know more about DV">DV</a>` <br/> `W=-2xx2.5=-"5 L atm"=-"506.3 J"`<br/> Because this work is used in raising the temperature of water, so work done is equalto the <a href="https://interviewquestions.tuteehub.com/tag/heat-21102" style="font-weight:bold;" target="_blank" title="Click to know more about HEAT">HEAT</a> supplied i.e., `w=q=m.c_(s).DeltaT` <br/> Given that, `m= 18g"(= 1 mole)", c_(s)=4.184g^(-1)K^(-1)`, <br/> `q=+506.3J, DeltaT=? `(Heat is given to water) <br/> `DeltaT=(q)/(c_(s).m)=(506.3)/(4.184xx18)=6.72` <br/> `therefore"<a href="https://interviewquestions.tuteehub.com/tag/final-461168" style="font-weight:bold;" target="_blank" title="Click to know more about FINAL">FINAL</a> temperature, "T_(f)=T_(i)+DeltaT=293+6.72` <br/> `=299.72K~~300K`</body></html>


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