H2(g) + I2(g) → 2HI(g) I was given this problem: A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in both the reactant H2 and product HI. Iodine is in Group VIIA, so it has an oxidation number of –1 in both the reactant I2 and product HI. Neither hydrogen nor iodine changes oxidation states, so the reaction is not a redox reaction. How can I describe the mistake that the student made, and determine whether or not the reaction is a redox reaction.
H2(g) + I2(g) → 2HI(g) I was given this problem: A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in both the reactant H2 and product HI. Iodine is in Group VIIA, so it has an oxidation number of –1 in both the reactant I2 and product HI. Neither hydrogen nor iodine changes oxidation states, so the reaction is not a redox reaction. How can I describe the mistake that the student made, and determine whether or not the reaction is a redox reaction.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.101PAE
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H2(g) + I2(g) → 2HI(g)
I was given this problem:
A student makes the following statements:
- Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in both the reactant H2 and product HI.
- Iodine is in Group VIIA, so it has an oxidation number of –1 in both the reactant I2 and product HI.
- Neither hydrogen nor iodine changes oxidation states, so the reaction is not a
redox reaction .
How can I describe the mistake that the student made, and determine whether or not the reaction is a redox reaction.
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