Giving the IUPAC name for Al2(Cr2O7)3 ?

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The IUPAC name for Al2(Cr2O7)3 is aluminum dichromate, as aluminum has a +3 oxidation state and dichromate has a -2 charge. For As2S3, it can be named either arsenic trisulfide or arsenic (III) trisulfide, with arsenic in a +3 oxidation state due to sulfur's -2 charge. The oxidation states are determined by the known charges of the elements involved. Understanding these oxidation states is crucial for correctly naming compounds. The discussion emphasizes the importance of recognizing oxidation states in IUPAC naming conventions.
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Homework Statement



I don't understand how to do this. There is 2 of them I am not sure of?

1st: As2S3 - Is the correct IUPAC name: DiAresenic Trisulfide?

2nd: Al2(Cr2O7)3 - IS it DiAluminum ... Need help with this. How do you get the IUPAC name from this. Any help would be great!



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The Attempt at a Solution

 
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1. Since we know sulfur is in a -2 oxidation state, that means arsenic is +3. So you could call it either arsenic trisulfide or arsenic (III) trisulfide.

2. Aluminum is always +3, and dichromate is always -2, so the name is aluminum dichromate.
 
I am still having trouble with As2S3

How do we know sulfur is in a -2 oxidation state? And how does Arsenic get a +3

How does that turn into Arsenic Trisulfide?

Really appreciate help on this! Thanks.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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