Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO3) at high temperature:CaCO3(s) → CaO(s) + CO2(g)In one particular reaction, 70 g of CaCO3 is heated at 450°C in a 5.0 L vessel. The pressure of CO2 is 0.24 atm after 4.0 minutes. What is the average rate of CO2 production in moles per minute during the 4 minutes? (Enter in mol/min.)If you assume this rate of decomposition remains constant, how many minutes will it take for the entire sample of CaCO3 to decompose?

This ia the part of gaseous state Here ideal equation may help to solve this. PV= nRT

Answered: CaCO3(s) → CaO(s) + CO2(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO₃) at high temperature:

CaCO₃(s) → CaO(s) + CO₂(g)

In one particular reaction, 70 g of CaCO₃ is heated at 450°C in a 5.0 L vessel. The pressure of CO₂ is 0.24 atm after 4.0 minutes. What is the average rate of CO₂ production in moles per minute during the 4 minutes? (Enter in mol/min.)

If you assume this rate of decomposition remains constant, how many minutes will it take for the entire sample of CaCO₃ to decompose?

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