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1 L of CO2 is passed through red hot coke. The volume becomes 1.4 L at same temperature and pressure. What is the composition of the product?

When carbon dioxide reacts with red hot coke, carbon monoxide is formed. The balanced chemical equation for this reaction can be written as:


`CO_2 + C -> 2CO`


Here, 1 mole of carbon dioxide reacts with 1 mole of coke to produce 2 moles of carbon monoxide. 


Let us assume that x liters of carbon dioxide are consumed in the reaction, then the remaining volume of carbon dioxide is 1-x liters.


Assuming STP conditions, 1...

When carbon dioxide reacts with red hot coke, carbon monoxide is formed. The balanced chemical equation for this reaction can be written as:


`CO_2 + C -> 2CO`


Here, 1 mole of carbon dioxide reacts with 1 mole of coke to produce 2 moles of carbon monoxide. 


Let us assume that x liters of carbon dioxide are consumed in the reaction, then the remaining volume of carbon dioxide is 1-x liters.


Assuming STP conditions, 1 l of CO2 = 1/22.4 moles


and x l = x/22.4 moles


Using stoichiometry,


x/22.4 moles of CO2 will produce 2x/22.4 moles of CO.


At STP, 2x/22.4 moles = 2x l (1 mole = 22.4 l at STP)


Thus, the final volume of gases will include the leftover CO2 and newly formed CO.


That is, 1-x + 2 x = 1.4 l


or, 1 + x = 1.4


or, x = 0.4 l


and 2x = 0.8 l


Thus, 0.8 l of CO are formed. And 0.6 l (= 1- x = 1- 0.4) of CO2 are left over.


Hope this helps. 

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