Reaction Stoichiometry, Gas Laws, Percent Composition 1) Determine the limiting

Question

Reaction Stoichiometry, Gas Laws, Percent Composition

1) Determine the limiting reactant and the theoretical yield (in g) of nitrogen that can be formed from 24.0 g N2O4 and 23.5 g N2H4 molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.

                                                                        N2O4(l) + 2 N2H4(l) 3 N2(g) + 4 H2O(g)

a)   Limiting Reactant_______________

b)   Theoretical yield of N2_________________

c)If 4.30 grams of N2 was actually produced determine the percent yield and the grams of each reactant which remain:

           Percent yield _____________________     

           Mass of each reactant remaining ___________________

If the above reaction took place in a sealed container, which of the gaseous products shown would have the higher mole fraction in the gas phase above the liquid solution?_________

      e) What volume would 4.30 g of Nitrogen gas occupy at STP? _________________

Explanation / Answer

Reaction Stoichiometry, Gas Laws, Percent Composition 1) Determine the limiting

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