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I think D
it was D
and why do you think its D??
it answer was D
i already passed
D seemed like the only logical one
alright .. well you did good... i had the same one on my test yesterday.. i also pick D and i got it right
lol did u already pass the class?
cuz im on the CST for the unit
yes with A
oh well its going to be hard ..
did u do it online?
no .. my school has it wibsit .. i forgot the name of it
well can u help me with a couple more question?
ill try my best . sure
Which of the following is an example of a galvanic cell? A. A cell with a nonspontaneous redox reaction B. A battery that has a negative voltage C. A cell that has energy added to it D. A battery that produces electricity
hmm let me think about that one ..
i would say D . a battery that produces electricity... sorry if i get it wrong .. i'm still working on cells
its k (:
i just appreciate the help
What is the oxidation state of S in S2O32-? A. +4 B. +2 C. +3 D. –2
The half-reactions and overall reaction for this voltaic cell are Zn(s) → Zn2+(aq) + 2 e– Eanode.. = –0.762 V Cu2+(aq) + 2 e– → Cu(s) Ecathode = 0.342 V Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Ecell = Ecathode – Eanode = 0.342 – (–0.762) = 1.104 V ... my teacher says think about this first ..
lmao lookin at that just throws me off more
oh sorry i know but it dose help alot
if i understood it i bet it would help alot
What is a redox reaction? A. A reaction in which protons have been transferred from one atom to another B. A reaction in which atoms have been transferred from one compound to another C. A reaction in which electrons have been transferred from one atom to another D. A reaction in which mass has been transferred from one reactant to another
do you know geometry?
i got this for my work class
I can help you on the last two questions you asked, if you still need it. Lets start with: What is the oxidation state of S in S2O32-? So, as you need to find the oxidation state of S, firstly we will need to find the oxidation state of O (oxygen). If you look on a periodic table, you will see that oxygen is in group 6. This means it has 6 valence electrons on its outer shell. Each element wants to have a full outer shell, just like the noble gases. A full outer shell of electrons consist of 8 electrons, so that means oxygen is 2 away from having a full shell. So, electrons have a negative charge, and the ion it forms has a full outer shell. So as we said before, oxygen needs 2 more electrons to be full. This means it charge will be 2, however we dont know if its a positive or negative charge yet. But, this is easy to figure out. Electrons are negative. If an element has more of a negative thing, it will have more of a negative charge. Same as if it had more protons, which have a positive charge, it would become more positive. Because oxygen NEEDS electrons, it will have more of a negative thing. So, now we know oxygen's oxidation number is -2. As you can see, in the compound there are 3 lots of oxygen (O3) so, we will have to times our charge by 3 (-2 x 3 = -6). So overall, the oxygens have a charge of -6. The charge on the overall compound is -2. Because compounds need a positive and negative to bond, we know S will have a positive charge. This means that we will need to keep 2- from our -6 we have on all our oxygens. So to work out the charge on S, we will basically have this equation: \[x + -6 = -2\] What will be needed to make -6 into -2? When you work this out (which is basic maths I'm sure you'll get it), that will be the charge of S.
And for this: What is a redox reaction? It is easy to remember this: OIL RIG Oxidation Is Loss (of electrons) Reduction is Gain (of electrons) It's always electrons that are being gained, or lost. Not protons, atoms or mass. So from this information you can figure out your answer. Sorry for the long explanation, I hope it helps you understand it better for the future :)