Asystem had 150 kj of work done on it and its internal energy increased by 60 kj. how much energy did the system gain or lose as heat?

The heat lost by the system from the given data is -110 kJ.

The given parameters;

The energy gained or lost by the system is calculated by applying the first law of thermodynamics as shown below;

ΔU = Q + W

where;

Q = ΔU - W

Q = 60 kJ - 150 kJ

Q = - 110 kJ

Thus, the heat lost by the system is -110 kJ.

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The system loses 90 kJ of heat

Explanation:

We can answer the question by using the 1st law of thermodynamics, which states that:

where

is the change in internal energy of the system

is the heat absorbed by the system (positive if absorbed, negative if released by the system)

is the work done by the system (positive if done by the system, negative if done by the surrounding on the system)

In this problem, we have:

is the work done (negative, because it is done by the surrounding on the system)

is the increase in internal energy

Using the equation above, we can find Q, the heat absorbed/released by the system:

And the negative sign means that the system has lost this heat.

1 - wave length

2 - amplitude

3 - crest

4 - trough

explanation:

duh.

be subject to a force andchange its motion