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Oxidation States of Elements

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1. Identify oxidation states of all elements.

3Ag(s) + 4HNOsub3(aq)->3AgNOsub3(aq)+NO(g)+2H2O(l)

I have everything except I thought O = -6 but it's wrong. Why?

2a)A 6.35L sample of gas is collected at 55degreeC and 0.892 atm. What volume of the occupy at 1.05 atm and 20.0degree C.

PV=nRT
(.892)(6.35)=n(o.o821)(55+273)

2b) If this gas weighs 4.237g, what monoatomic gas is it?

3) Write the molecular and net ionic reactions for the following combinations of reactants. If a precipate does not form, write the molecular equation with the proper phases, followed by "no reaction" for the net ionic equation.

A. Beryllium sulfate and rubidium chloride.

Molecular equation:

BeSOsub4(aq) +2RbCl(aq) -> BeClsub2(s) + Rbsub2SOsub4(aq)

Now, told in BeClsub2(s) the solid is wrong--why..what is it aqueous???

B. Cobalt(II) nitrate and lithium sulfide

Do molecular equation showing all states and charges

Do the net ionic equation showing all states and charges and balance it.

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Solution Summary

The solution explains, in words or calculations as necessary why the oxidation state of oxygen in the given reaction is not -6 and then goes on to tackle the questions of ideal gas pressures and net ionic reactions in a similarly clear manner.

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Question 1

Oxidation states of the oxygen. What's going on? The oxidation state of oxygen is not -6. It is -2. You're forgetting that there are three oxygen atoms in NO3. Therefore, the oxidation state of each oxygen is -2, although as you know, the ...

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