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The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 4.60 g NO is formed? Pb(NO3)2 (s) → PbO (s) + NO2 (g) + O2 (g) please show all the work

Respuesta :

transitionstate

Answer:

            0.8 g of O₂

Solution:

             The balance chemical equation is as follow,

                         2 Pb(NO₃)₂      →     2 PbO + 4 NO₂ + O₂

According to equation,

     184 g (4 moles) NO₂ is produced along with  =  32 g (1 mole) O₂ gas

So,

    4.60 g NO₂ when formed will produce along  =  X g of O₂

Solving for X,

                     X  =  (32 g × 4.60 g) ÷ 184 g

                     X  =  0.8 g of O₂

kenmyna
the  moles  of oxygen produced when 4.60 g No2  is  formed is calculated as below

find the moles of NO2 =  mass/molar mass
= 4.60g/46 g/mol = 0.1  moles

2Pb(NO3)2 = 2PbO +4 NO2 +O2

by use of mole ratio between  No2 to O2  which is  4:1 the moles  of  O2
=  0.1 x1/4 = 0.025moles

mass  of O2 = moles x  molar mass

= 0.025  moles  x  32 g/mol = 0.8 grams  of oxygen

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