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du=dq+dw So our first law, du is dq plus dw.
热力学第一定律。
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We're still going to be able to write that dq=0 it's an adiabat so that dq equals zero.
绝热条件依然成立,于是。
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Well, dq is equal to zero and dw is equal to zero dq=0 dw=0 because it's isolated.
隔离的孤立系统,这时。
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dq=0 But if it's adiabatic, then dq is equal zero, du=dw and for an adiabatic process, then du is equal to dw.
但如果它是绝热的，那么，因此对于绝热过程。
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If you want to have an infinitestimally small change, you end up writing dh is dq sub p.
这是对于有限的变化而言的,如果是一个无限小的变化。
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dU=dq+dw Well from the first law, du is equal to dq plus dw, and I wrote down everything I knew at the beginning here.
第一定律“,前面我们已经,看到了。
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So what we've discovered from this relationship dq that du at constant volume is equal to dq v.
从这个关系式里我们发现,恒体积时的du等于恒体积时的。
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dq It's an ideal gas in adiabatic expansion 0 dq is equal to zero.
说明,等于。
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One is, du, u is called the internal energy dw or just the energy, is equal to dq plus dw.
其中一个是：du，u是内能,或能量，等于dq加上。
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Cp, I forgot to put my little bar on top here because it's per mole Cp dT that's my dq here.
上面的Cv我忘记加上横线了,因为它也是摩尔热容。
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I can substitute dq from this expression in here.
代入这个表达式的这里。
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dU=dq+dw Still know that du is dq plus dw.
所以。
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dq=0 dw=-pdV I wrote dq equals zero I wrote what dw was.
这样的式子。
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dq=0 Let's write that down. dq equals zero.
它说明。
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dq=CvdT STUDENT: PROFESSOR BAWENDI: Well, let's see.
学生：在等容过程中：,对理想气体。
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TdS It comes from the fact that dq reversible is T dS, pdV and dw reversible is minus p dV.
这个结论来自于：可逆过程下dq等于，做功dw等负的。
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dq is zero. The that is adiabatic.
条件不同。
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Adiabatic means dq equals zero.
首先是“绝热“
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And for the spontaneous change which happens irreversibly That means that'll be dq irreversible.
对于不可逆的自发过程,这说明dq是不可逆的,当过程是可逆时。
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Going around in a cycle the integral of dq over T is less than or equal to zero.
对一个循环过程作dq除以T的积分,小于等于零。
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if it's a reversible process then the equality holds, but if it's irreversible, which means it happens spontaneously, T then dS is greater than this.
对于可逆过程，等号成立，但是如果是不可逆过程，这些不可逆过程是自发进行的，那么dS大于dq除以。
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du=0 So du is equal to zero because dq and dw are both zero.
因此,因为dq和dw都等于零。
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We saw that in general dS is greater than T or equal to dq over T.
我们发现一般来说dS大于,或者等于dq除以。
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Adiabatic q equal to zero. It's also delta H 0 which is zero. The two didn't necessarily follow because remember, delta H is dq so p is only true for a reversible constant pressure process.
在这个过程中ΔH等于,绝热的所以q等于0，而ΔH也等于,这两个也不一定有因果关系,因为，记住，ΔH等于dq只有在恒压。
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Over here, we have dq=Cp dT, the heat, the proportionality between heat - and temperature rise is given by this, the constant pressure heat capacity.
这里我有dq=CpdT，这是热量，这是联系热量,和温度变化的系数，恒压热容。
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T Namely dS is greater than dq over T.
换句话说就是dS大于dq除以。
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T That dS is greater than dq over T.
对吗，熵的变化dS大于热量dq除以温度。
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