In this chapter, we used a simpliied equation for the combustion of gasoline. Bu

Question

In this chapter, we used a simpliied equation for the combustion of gasoline. But the products generated in the operation of real automobile engines include various oxides of nitrogen, and it is desirable to remove these compounds from the exhaust stream rather than release them into the atmosphere. Currently, this is done by the "catalytic converter," but other technologies are being explored. One possible method involves the use of isocyanic acidm HNCO, which reacts with NO2 to produce N2, CO2, and H2O, as shown in the equation below :

8HNCO +6NO2 --> 7N2 + 8CO2+ 4H2O

What mass of HNCO would be required to react completely with the estimated 1.7 x 10^10 kg of NO2 produced each year by U.S automobiles? How might the fact that the reaction above produces CO2 affect its feasibility for this application?

Explanation / Answer

Mass of NO2 produced by U.S.automobiles each year = 1.7*10^10 kg

=> No.of moles of NO2 produced by U.S.automobiles each year = 1.7*10^10 / 46 = 3.69*10^8 kilo moles

=> no.of moles of HNCO required = No.of moles of NO2 * (8/6) = 4.92*10^8 kilo moles

=> Mass of HNCO required = (4.92*10^8)*43 = 2.12 * 10^10 kg

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