The figure (Figure 1) shows a p V diagram for an ideal gas in which its pressure

Question

The figure (Figure 1) shows a pV diagram for an ideal gas in which its pressure tripled from a to b when 651J of heat was put into the gas.

How much work was done on or by the gas between a and b?

Without doing any calculations, decide whether the temperature of this gas increased, decreased, or remained the same between a and b. Explain your reasoning.

By how much did the internal energy of the gas change between a and b ?

Did it increase or decrease?

What is the temperature of the gas at point b in terms of its temperature at a , Ta

Explanation / Answer

p1=0.75 atm =0.75*1.013*10^5 Pascal

=7.5975*10^4 pascal

p2=3*0.75=2.25 atm

=22.7925*10^4 pascal

v1=v2=0.025 m^3

a)

work done on or by the gas between a to b is Zero( because volume is constant)

b)

temperature increases because from pv=nRT

if p increases then T increases

c)

dQ=651 J

dQ=dU+dw

651=dU+0

dU=651 J

d)

increases

e)

at point a temparature is Ta

at point b temparature is Tb

and let Cv be specific heat of gas n mole of given idealgas

dU=n*Cv*(dT)

651=n*Cv*(Tb-Ta)

Tb=Ta+[651/(n*Cv)]

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