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1. Calculate the mass of NO2 formed from 3.00 kg of ammonia in Reaction 2 assuming
an 80.0% yield.

3000 / 17
176.5
176.47 × 46 = 8117.62
8117.62 × 80 / 100 ( = 6494 g)
6494 / 1000 = 6.5

why do you multipy by 46?

Thank you
2. (Original post by Elizabeth138)
Calculate the mass of NO2 formed from 3.00 kg of ammonia in Reaction 2 assuming
an 80.0% yield.

3000 / 17
176.5
176.47 × 46 = 8117.62
8117.62 × 80 / 100 ( = 6494 g)
6494 / 1000 = 6.5

why do you multipy by 46?

Thank you
46 is the Mr of NO2

Also try to include the units in your working out so it's very clear exactly what you're doing, and it's just a very good habit to get into anyway
3. (Original post by KaylaB)
46 is the Mr of NO2

Also try to include the units in your working out so it's very clear exactly what you're doing, and it's just a very good habit to get into anyway
Thank you!

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Updated: January 4, 2017
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