Because of this difference in entropy change, the net entropy change of the entire system is ________ during a real isothermal e
1 answer:
Answer:
The net entropy change of the entire system is increasing during a real isothermal expansion.
Explanation:
The net entropy of a system is always zero for reversible process, and it is positive for irreversible process. It is also important to notice that the net entropy is the change of total entropy, that means.
In a reversible isothermal process the total entropy change is 0, where the increase of entropy of the system has the same magnitude as the decrease of the entropy of the surroundings.
But in a real isothermal process the magnitude of the entropy lost by the surroundings is less than the magnitude of entropy gained by the system, thus we have irreversible process so the net entropy is always positive.
In case of a gas for example where we have isothermal expansion, the work done is by the gas, causing a heat loss by the surroundings. It is that temperature difference that will make the entropy lost by the surroundings less than the magnitude of entropy gained by the gas.
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Answer:
Explanation:
Hello,
Considering the ideal equation of state:
The moles are defined in terms of mass as follows:
Whereas the gas' molar mass, thus:
Now, since the density is defined as the quotient between the mass and the volume, we get:
Solving for :
Thus, the result is given by:
Best regards.
Answer:
You need 8,324 g of CaCl₂ yo make this solution
Explanation:
Molarity is a way to express concentration in a solution, in units of moles of solute per liter of solution.
To know the grams of CaCl₂ it is necessary to know, first, the moles of this substance with the desired volume and concentration , thus:
0,1500 L × = 0,075 CaCl₂ moles
Now, with the molar mass of CaCl₂ you will obtain the necessary grams, thus:
0,075 CaCl₂ moles × = 8,324 g of CaCl₂
So, you need <em>8,324 g of CaCl₂</em> to make 150,0 mL of a 0,500M solution
I hope it helps!