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Yuri [45]
3 years ago
9

Heat is added to an open pan of water at 100.0°c, vaporizing the water. the expanding steam that results does 43.0 kj of work, a

nd the internal energy of the system increases by 604 kj. how much energy is transferred to the system as heat?
Physics
2 answers:
vampirchik [111]3 years ago
6 0
Heat = change in internal energy + Work done The internal energy of a system = heat added and mechanical work done by the system, i.e. U = Q + W rearranging the formula above, will give us: Q = deltaU + W 
Q = U - W = 604 kJ - 43.0 kJ = 561,000 J would be the answer.
PIT_PIT [208]3 years ago
4 0

Answer:

Heat transferred to the gas is given as

Q = 647 kJ

Explanation:

As per first law of thermodynamics we know that

Q = \Delta U + W

now here we know that

change in internal energy of the gas is

\Delta U = 604 kJ

Also the steam expands so we will have

W = 43 kJ

since volume increases to here work is done by the gas

now from above equation the heat given to the system is

Q = 604 + 43 = 647 kJ

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