Each is false explain why a. In any type of process, if a perfect gas absorbs heat, its temperature must rise.b. The values of work (w) and heat (q) will always be equal and opposite no matter the type of process thatoccurs.c. AH can only be calculated for a process in which the pressure of the system is held constant.d.In an adiabatic expansion, the system transfers heat to the surroundings.e. The enthalpy of formation value, AfHº, for a molecule is the absolute amount ofwithin that molecule.energy contained

(a). From the first law, ΔU=Q−WΔU=Q−W. If the process is isothermal, then ΔU=0 (assuming an ideal…

Answered: a. In any type of process, if a perfect…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Each is false explain why

a. In any type of process, if a perfect gas absorbs heat, its temperature must rise.
b. The values of work (w) and heat (q) will always be equal and opposite no matter the type of process that
occurs.
c. AH can only be calculated for a process in which the pressure of the system is held constant.
d.
In an adiabatic expansion, the system transfers heat to the surroundings.
e. The enthalpy of formation value, AfHº, for a molecule is the absolute amount of
within that molecule.
energy contained

Expert Solution

Step 1

(a). From the first law, $Δ U = Q - W$ . If the process is isothermal, then $Δ U = 0$ (assuming an ideal gas), so Q = W. The heat energy is consumed by your gas doing work, so there is no change in internal energy (temperature). That's why statement is false

(b).

The first law of thermodynamics states that the change in internal energy of a system equals the net heat transfer into the system plus the net work done on the system W. In equation form, the first law of thermodynamics is,

form, the first law of thermodynamics is,

delta, U, equals, Q, plus, W

Wait, why did my book/professor use a negative sign in this equation?

Here delta, U is the change in internal energy U of the system. Q is the net heat transferred into the system—that is, Q is the sum of all heat transfer into and out of the system. W is the net work done on the system.

So positive heat Q adds energy to the system and positive work W adds energy to the system. This is why the first law takes the form it does, simply says that you can add to the internal energy by heating a system, or doing work on the system.

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