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Hi guys and gals. I'm new to the site and have been reading and learning a lot from here. I can't believe I didn't know about this place before. Anyway I'm having a pretty difficult time with a certain reaction that I had to do in my General Chemistry lab. Any help would be appreciated!

We were asked to add H

There are actually 2 that are giving me problems and I've been sitting here staring at them for about an hour now. I just can't seem to get it right.

1. KI

2. K

I just can't get an equation that seems right to me.

1. according to the lab manual, just adding the sulfuric acid to the potassium iodide at room temp you should see effervescense and a darkening of the solid, then you should smel hydrogen sulfide and see violet fumes of Iodine.

So my take on it is as follows;

2KI

The balancing seems to work out for this one but I am unsure if I have the states correct and if that is really the appropriate equation (I did a google search and saw stuff like SO

2. Our instructor provided us with a formula on the board as follows;

2CrO

so my thought was that because K

Thank for any help you guys can offer!

We were asked to add H

_{2}SO_{4}_{(aq)}to a bunch of different salts, watch for the physical manifestations of the reactions (if there were any) and then write a balanced equation/net ionic equation.There are actually 2 that are giving me problems and I've been sitting here staring at them for about an hour now. I just can't seem to get it right.

1. KI

_{(s)}+ H_{2}SO_{4}_{(aq)}2. K

_{2}CrO_{4}_{(s)}+ H_{2}SO_{4}_{(aq)}I just can't get an equation that seems right to me.

1. according to the lab manual, just adding the sulfuric acid to the potassium iodide at room temp you should see effervescense and a darkening of the solid, then you should smel hydrogen sulfide and see violet fumes of Iodine.

So my take on it is as follows;

2KI

_{(s)}+ H_{2}SO_{4}_{(aq)}-> I_{2}_{(g)}+ H_{2}S_{(g)}+ 2K^{+}_{(aq)}+ 2O_{2}_{(g)}The balancing seems to work out for this one but I am unsure if I have the states correct and if that is really the appropriate equation (I did a google search and saw stuff like SO

_{2}as a possible product)2. Our instructor provided us with a formula on the board as follows;

2CrO

_{4}^{2-}+ H_{2}O -> Cr_{2}O_{7}^{2-}+ 2OH^{-}so my thought was that because K

_{2}CrO_{4}is an ionic compound it should dissociate upon addition of solvent but I just can't make the reaction work out on paper. It seems from what the instructor said the chromate should become dichromate and there should be a hydroxide product but, for the life of me, I can't figure out what the acid is doing in the reaction. It seems like whatever available water in the acid solution is reacting with chromate but then what happens to the hydrogen and sulfate ions? Are they spectators? I really just can't wrap my head around this problem. I feel as though there is some kind of information, or key concept, that I have not been taught yet because I just can't come up with an answer that sits right with me.Thank for any help you guys can offer!

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