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The equation below shows the decomposition of lead nitrate. how many grams of oxygen are produced when 11.5g NO2 is formed? 2Pb(NO3)2(s) -> 2PbO(s) + 4NO2(g) + O2(g) a. 2.88 g b. 2.00 g c. 32.0 g d. 1.
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The equation below shows the decomposition of lead nitrate. how many grams of oxygen are produced when 11.5g NO2 is formed?

2Pb(NO3)2(s) -> 2PbO(s) + 4NO2(g) + O2(g)

a. 2.88 g
b. 2.00 g
c. 32.0 g
d. 1.00 g

PLEASE AND THANK YOU IN ADVANCE

User Panji Gemilang
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1 Answer

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Number of moles of NO2 = 11.5/(14+16x2) =0.250mol
Mole ratio: 4NO2 to 1O2
Number of moles of O2=0.250/4 =0.0625mol
Mass of O2 produced= 0.0625x32 =2g
Answer: B
User Blaine
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