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4 years ago

13

Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.0

0 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L∙atm)

1 answer:

Alexxandr [17]4 years ago

7 0

Explanation:

The given data is as follows.

q = -25.0 kJ, Pressure (P) = 1.50 atm

$\Delta V$ = (12 - 6) L = 6 L

Therefore, product of pressure and change in volume will be as follows.

$P \Delta V = 1.50 atm \times 6 L$

= 7.5 L atm

= $7.5 \times 101.3$

= 759.75 J

Now, we will calculate the change in internal energy as follows.

$\Delta E = q + w$

= $q + P \Delta V$

= -25000 kJ + 759.75 J

= 24240.25 J

or, = 24.240 kJ (as 1 kJ = 1000 J)

Thus, we can conclude that the change in internal energy ( $\Delta E$ ) for a system is 24.240 kJ.

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