Question

12 moles of C(s) reacts with 9 moles of O2(g) to form CO(g) and CO2(g). If no reactant remains, then calculate the density of the final gas mixture (in g/L) at a temperature of 360 K and a pressure of 1.642 atm. (R = 0.0821 L·atm/mol·K)

Name: 12 mole cs reacts with 9 mole of o2 g to form co g and co2 g if no one reactant remains then calculate the density of final gas mixture in gl at 360 k temperature and 1642 atm pressure r 008 27316
Uploaded: 2023-06-30T20:14:40-08:00
Duration: 1 min 47 s
Channel: Adi S
Description: 12 mole cs reacts with 9 mole of o2 g to form co g and co2 g if no one reactant remains then calculate the density of final gas mixture in gl at 360 k temperature and 1642 atm pressure r 008 27316

          12 moles of C(s) reacts with 9 moles of O2(g) to form CO(g) and CO2(g). If no reactant remains, then calculate the density of the final gas mixture (in g/L) at a temperature of 360 K and a pressure of 1.642 atm. (R = 0.0821 L·atm/mol·K)

Added by Jared A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

06/30/2023

Step 1

The balanced chemical equation for the reaction is: $$C(s) + O_2(g) \rightarrow CO(g)$$ $$C(s) + 2O_2(g) \rightarrow CO_2(g)$$ For the first reaction, the mole ratio of C to O2 is 1:1. For the second reaction, the mole ratio of C to O2 is 1:2. For the first Show more…

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12 moles of C(s) reacts with 9 moles of O2(g) to form CO(g) and CO2(g). If no reactant remains, then calculate the density of the final gas mixture (in g/L) at a temperature of 360 K and a pressure of 1.642 atm. (R = 0.0821 L·atm/mol·K)