change in eternal energy= n*Cv*delta T n= moles Cv= molar specific heat of gas at constant volume Delta
Δu = q- w
the system has been given internal energy of 640j and the work system does on surroundings is 260j. therefore by first law of thermodynamics the internal energy of system increases by (640-260=380)j.
The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to; 430 J = 120 J + (internal energy change) so Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
-15.2 J
Assuming you are talking about a closed system, it is the difference in energy transferred to or from the system as work and HEAT.
If the internal energy of the system increases the temperature will increase.
the system has been given internal energy of 640j and the work system does on surroundings is 260j. therefore by first law of thermodynamics the internal energy of system increases by (640-260=380)j.
Internal energy is an extensive state function. That means it depends on how much of a substance you have but if you fix the composition, pressure, temperature, volume, and (in the case of a system at a phase equlibrium point, like water at the freezing point) the phase of a system, the specific internal energy will be constant. If you take a closed system and change the volume of it, you will be doing work (or allowing the system to do work) and the internal energy can change - so - yes - internal energy of a system depends upon volume. Also, if you fix the composition, temperature, pressure, and phase of a homogeneous mass but change the volume, you will increase the amount of mass you included in the system, thus changing the total internal energy (because it is, after all, an extensive function).
dU=q-w where dU is the differential change in internal energy q is the differential quantity of heat added to a system w is the differential quantity of work done by a system on its surroundings
5.155
The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to; 430 J = 120 J + (internal energy change) so Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
-15.2 J
The formation of bonds causes an energy release, while the breaking of bonds causes an absorption of energy. In a combustion reaction c+o2 --> co2, the reactants have a higher internal energy than the products resulting in a negative internal energy because energy is flowing out of the system to the surroundings. However in co2 ---> c+o2, the reactants have a lower internal energy than the products, so the internal energy of the system is positive as energy is flowing into the system from the surroundings.
Assuming you are talking about a closed system, it is the difference in energy transferred to or from the system as work and HEAT.
-70 Joules
If the internal energy of the system increases the temperature will increase.
* First law of thermodynamics, about the conservation of energy: : :: The change in the internal energy of a closed thermodynamic system is equal to the sum of the amount of heat energy supplied to the system and the work done on the system. --from Wikipedia
In general Conservation of Energy does not hold internal to a system, it only holds at the boundary of the system. This is where the limits of the system are. Internal to the system energy is not conserved. The situations where the Conservation does not apply is where the force is not zero or the first derivative of energy is not zero.