Limestone (CaCO3) decomposes upon heating to yield quicklime (CaO) and carbon dioxide. At what temperature does limestone exert a decomposition pressure of 1 bar?
Added by Irene W.
Step 1
According to Le Chatelier's principle, the equilibrium will shift to the right (towards the products) as the temperature increases, resulting in an increase in the partial pressure of CO2. The exact temperature at which the decomposition pressure of limestone Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 96 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Limestone (CaCO3) is decomposed by heating to quicklime (CaO) and carbon dioxide. Calculate how many grams of quicklime can be produced from 1.54 kg of limestone
Madhur L.
Limestone (CaCO3) is decomposed to CaO and CO2 by heating. How many grams of CaO can be produced from 1.0 kg of limestone? What is the percentage yield of the reaction if 0.5 kg of CaO is obtained?
Ma Ednelyn L.
If $10.11 \mathrm{~g}$ of limestone decomposes by heat to give $8.51 \mathrm{~g}$ of solid calcium oxide and carbon dioxide gas, what is the mass of carbon dioxide produced?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD