Hi All, once again I'm stuck. Here's the question.
Antimony is a grey metalloid. It is usually found in the mineral stibnite Sb2S3. Pure antimony can be obtained in either of two ways:
(i) Stibnite is reacted with iron
(ii) Two reaction occur
1) Stibnite reacts with oxygen in a process called roasting, which forms antimony (IV) oxide (Sb2O4), and sulfur dioxide.
2) The antimony (IV) oxide is then reacted with carbon to displace solid antimony from the compound.
a) Predict the products of the first method of extraction. Write a balanced chemical equation to represent the process. Classify the reaction.
b) Write a balanced equation for the process of roasting in the second method.
c) Predict the products of the second reaction of the second method, and represent the reaction in a balanced chemical equation. (Remember the whole goal is to obtain pure antimony.
My answers are:
a) Sb2S3 + Fe ---> FeS3 + Sb2
**Single Displacement Reaction
b) Sb2S3 + 2O2 ---> Sb2O4 + S3
c) Sb2O4 + 4C2 ---> 4C2O + Sb2
Could someone point out any errors which I've made, thanks.