The reaction NO₂(g)+ CO(g)$\to$ NO(g)+ CO₂(g)appears to be second order in NO and zero order in CO,with a rate constant at 488 K of 0.749 M^-1s^-1.Suppose the initial partial pressure of NO₂ in a reaction vessel containing air at STP (1atm,273 K)is 0.0278 atm.How many moles of NO₂ are present per liter after 2.50 minutes?

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The Answer of The reaction NO₂(g)+ CO(g)$\to$ NO(g)+ CO₂(g)appears to be second order in NO and zero order in CO,with a rate constant at 488 K of 0.749 M^-1s^-1.Suppose the initial partial pressure of NO₂ in a reaction vessel containing air at STP (1atm,273 K)is 0.0278 atm.How many moles of NO₂ are present per liter after 2.50 minutes?

The Reaction NO2(g)+ CO(g) →\to→ NO(g)+ CO2(g)appears to Be Second Order in NO and Zero

The Reaction NO₂(g)+ CO(g) $\to$ NO(g)+ CO₂(g)appears to Be Second Order in NO and Zero