Nitric acid and magnesium reaction, slow gas production

Click For Summary
SUMMARY

The reaction between magnesium and nitric acid produces hydrogen gas at a slower rate compared to magnesium's reaction with hydrochloric acid. This is attributed to nitric acid's dual role as a strong oxidant, which may lead to the formation of nitrogen oxides instead of hydrogen gas. The reaction can be represented by the equation Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g), but the presence of nitrogen oxides complicates the expected outcome. Additionally, hydrogen may react with nitric acid, reducing it to ammonia, further decreasing hydrogen gas production.

PREREQUISITES
  • Understanding of acid-base reactions, specifically with strong acids like nitric acid.
  • Knowledge of oxidation-reduction reactions involving metals and acids.
  • Familiarity with the chemical properties of magnesium as a reductant.
  • Basic grasp of nitrogen oxides and their formation in chemical reactions.
NEXT STEPS
  • Research the formation and properties of nitrogen oxides in acid-metal reactions.
  • Study the differences in reactivity between nitric acid and hydrochloric acid with magnesium.
  • Learn about the reduction of nitric acid to ammonia in the presence of hydrogen.
  • Explore the kinetics of gas production in acid-metal reactions to understand rate variations.
USEFUL FOR

Chemistry students, educators, and researchers interested in reaction kinetics and the behavior of metals in acidic environments.

mbeaumont99
Messages
3
Reaction score
0

Homework Statement


I need to work out what is happening with the above reaction. Why is my data showing a very slow hydrogen gas production rate (if it even is hydrogen gas), in fact, even slower than the production of hydrogen gas from the reaction of magnesium and ethanoic acid. All acids used were 1 mol/L. Magnesium ribbon used had (roughly) the same surface area and mass.

Homework Equations


Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)

The Attempt at a Solution


With nitric acid being a strong acid and magnesium being a reactive metal surely the hydrogen gas production would be very high, just like that of HCl with magnesium. Magnesium is a strong reductant and nitric acid is a strong oxidant, could this be what is causing a problem with the reaction. I read on wiki that this COULD be due to the reaction producing nitrogen oxide (+1, +2, or +4 oxidation states for nitrogen - different sources giving different nitrogen oxides). Why would nitric acid and magnesium reacting produce a different gas to hydrogen at such a slow rate. I would really appreciate help with determining why this outcome has occurred. Thanks
 
Physics news on Phys.org
Perhaps hydrogen is reacting with the nitric acid reducing it to ammonia.
 

Similar threads

Magnesium Carbonates Reaction Under Various Test?
  • · Replies 1 ·
Replies
1
Views
3K
Why Does Adding Nitric Acid to Copper and Carbon Dioxide Produce Brown Gas?
  • · Replies 14 ·
Replies
14
Views
3K
Analyzing Oxygen Ratios in Magnesium Oxide Lab Reactions
  • · Replies 10 ·
Replies
10
Views
18K
How to determine strong acids when reacting with magnesium?
  • · Replies 3 ·
Replies
3
Views
3K
Chemistry Comparing methods of computing pH at equivalence point in titration
  • · Replies 4 ·
Replies
4
Views
2K
Acid-Base Reaction: Hydrochloric Acid and Magnesium Oxide Formula
  • · Replies 5 ·
Replies
5
Views
15K
What will be the product of this organic reaction?
  • · Replies 28 ·
Replies
28
Views
5K
Representing the Rate of Production?
  • · Replies 4 ·
Replies
4
Views
3K
How Much Hydrogen Gas Is Produced in a Magnesium and Hydrochloric Acid Reaction?
  • · Replies 2 ·
Replies
2
Views
3K
Triple electrode cell for energy storage and H2 production
  • · Replies 1 ·
Replies
1
Views
2K