Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Shadow on October 10, 2013, 01:12:53 PM
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I got very confused by studying this. I could really use some good explanation. For example, the equivalent unit of K2Cr2O7 is 1/6K2Cr2O7. If in a solution nK2Cr2O7=0.1mol, we should have 6 times more of 1/6K2Cr2O7 because 6*1/6=1, but it's not true. Please help :'(.
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labelling "equivalent" without specifying what something should be equivalent to is meaningless
hence your confusion
your example would be relevant in redox reactions with K2Cr2O7 , where each chromium went from + VI to + III , and the substance oxidized would supply one electron each: here the molar ratios, i.e. "the equivalent" would be 1:6
... but you have to specify this
regards
Ingo
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That's not the point of my confusion. I have meant for the situation you wrote.
Now, can you explain the thing I asked at the beginning?
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I got very confused by studying this. I could really use some good explanation. For example, the equivalent unit of K2Cr2O7 is 1/6K2Cr2O7. If in a solution nK2Cr2O7=0.1mol, we should have 6 times more of 1/6K2Cr2O7 because 6*1/6=1, but it's not true. Please help :'(.
Unless I am missing something, you got it reversed. If it is 1/6, then to get 1 equivalent you need 1/6 of the mole, not 6 moles.