Please answer both parts. Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is: 2H2O(g)⟶2H2(g)+O2(g) Calculate how many grams of O2(g) can be produced from 31.8 g H2O(g).  Consider the reaction. 2Pb(s)+O2(g)⟶2PbO(s) An excess of oxygen reacts with 451.4 g of lead, forming 314.6 g of lead(II) oxide. Calculate the percent yield of the reaction.

Question

Please answer both parts.

Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water.

The equation for the reaction is:

2H2O(g)⟶2H2(g)+O2(g)
  1. Calculate how many grams of O2(g) can be produced from 31.8 g H2O(g). 

Consider the reaction.

2Pb(s)+O2(g)⟶2PbO(s)
  1. An excess of oxygen reacts with 451.4 g of lead, forming 314.6 g of lead(II) oxide. Calculate the percent yield of the reaction.

 

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