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Test 2

Posted: Sun Mar 03, 2019 12:00 pm
by 204929947
Okay, so for Test 2, it had us put the redox molecules from increasing order, how would we do that?

Re: Test 2

Posted: Sun Mar 03, 2019 12:53 pm
by Kenan Kherallah 2C
You would look at the reducing power which is another way of saying how likely the substance is to be oxidized. This means the more negative the E potential the better.

Re: Test 2

Posted: Sun Mar 03, 2019 12:54 pm
by Henry_Phan_4L
So the one with better oxidizing power is the most positive one?

Re: Test 2

Posted: Sun Mar 03, 2019 1:26 pm
by Jonathan Zhao 4H
Yes, correct. The more positive the E value, the stronger the oxidizing power.

Re: Test 2

Posted: Wed Mar 06, 2019 12:16 pm
by shouse1f
On test 2 for another part of the same question it asked which 2 species would give the largest E cell, how do you determine this?

Re: Test 2

Posted: Wed Mar 06, 2019 12:50 pm
by Tatum Keichline 2B
More negative E for reducing and more positive E for oxidizing I believe

Re: Test 2

Posted: Wed Mar 06, 2019 2:22 pm
by sonalivij
The half reaction with the most negative standard potential is the strongest reducing agent, and the half reaction with the most positive standard potential is the strongest oxidizing agent

Re: Test 2

Posted: Wed Mar 06, 2019 9:29 pm
by Selina Bellin 2B
more positive e value corresponds to a higher oxidizing power