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OTP to be sent to Change
here we shall use the first law of thermodynamics
ΔQ = ΔU + ΔW
so, change in internal energy will be
ΔU = ΔQ - ΔW
here,
ΔQ = mL =1g x 540Cal/g = 540 Cal
ΔU = change in internal energy (to be calculated)
ΔW = change in work done
so,
ΔW = pΔV
where
ΔV = 1671cm3 - 1cm3 = 1670cm3 = 1670 x 10-6 m3
p = hρg = 0.76 x 13600 x 9.8 ~ 101293 N/m2
ΔW = 101293 x 1670x10-6 = 169.16J
or
ΔW = 169.16 / 4.2 = 40.3 Cal
thus, we have
ΔU = 540 Cal - 40.3 Cal
ΔU = 499.7 Cal = 2098.74 J
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