3Ag(s) + 4HNOsub3(aq)->3AgNOsub3(aq)+NO(g)+2H2O(l)
I have everything except I thought O = -6 but it's wrong. Why?
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.
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.
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 ...
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.