The change in the internal energy:-870 J
The laws of thermodynamics 1 state that: energy can be changed but cannot be destroyed or created
The equation is:
[tex]\rm \Delta U=Q+W[/tex]
Energy owned by the system is expressed as internal energy (U)
This internal energy can change if it absorbs heat Q (U> 0), or releases heat (U <0). Or the internal energy can change if the system does work or accepts work (W)
The sign rules for heat and work are set as follows:
• The system receives heat, Q +
• The system releases heat, Q -
• The system does work, W -
• the system accepts work, W +
Heat can be calculated using the formula:
Q = mc∆T
A 225 Delivers System J Of Heat To The Surroundings While Delivering 645 J Of Work, then
Q release heat = -225 J
The system does work, W = -645 J
the change in the internal energy, ∆E, of the system
∆E / ∆U = Q + W
∆E / ∆U = -225 - 645
∆E / ∆U = -870 J
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The change in the internal energy of the system is -870 J.
The given parameters;
The change in the internal energy of the system is calculated by applying the first law of thermodynamic as shown below;
ΔU = Q - W
where;
Substitute the given parameters and solve for change in internal energy;
ΔU = (-225) - 645 J
ΔU = -870 J
Thus, the change in the internal energy of the system is -870 J.
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