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Problem: The emission of NO2 by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the following reaction:2 CO(NH2)2(g) + 4 NO(g) + O2(g) → 4 N2(g) + 2 CO2(g) + 4 H2O(g)Suppose that the exhaust stream of an automobile has a flow rate of 2.51 L/s at 653 K and contains a partial pressure of NO of 12.1 torr. What total mass of urea is necessary to react completely with the NO formed during 8.1 hours of driving?

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PV=nRT

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The emission of NO2 by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the following reaction:
2 CO(NH2)2(g) + 4 NO(g) + O2(g) → 4 N2(g) + 2 CO2(g) + 4 H2O(g)
Suppose that the exhaust stream of an automobile has a flow rate of 2.51 L/s at 653 K and contains a partial pressure of NO of 12.1 torr. What total mass of urea is necessary to react completely with the NO formed during 8.1 hours of driving?

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Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.