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sulfuryl cholorie decomposes toSo2 and cl2
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Sulfuryl chloride, SO2Cl2, decomposes to SO2 and Cl2 according to the reaction
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b. ln*(No/N) = kt No = 100 N = 25 k is given Solve for t.
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Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?
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Isn't the rate -d(Cl2)/dt and -(1/3)d(F2)/dt? If that is so, then -d(Cl2)/dt = -(1/3)d(F2)/dt and
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Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?
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of those E looks like the best option but it should be: -d(Cl2)/dt=-1/3[d(F2)/dt]
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Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?
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You have not told us what the "following reaction" is. That makes all the difference.
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Place the following in order of decreasing molar entropy at 298 K.
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The order of decreasing molar entropy at 298 K is: F2 > Cl2 > H2
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To solve these problems, we'll need to use the given information and apply the principles of
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At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=>
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I think you need more information. Do you have a number of moles? a volume? pressure? 1. (Cl2) = 0;
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