Stoichiometry Question 2?
Part 1). Some rocket engines use a mixture of hydrazine (N2H4) and hydrogen peroxide (H2O2) as the propellant. The reaction is given by N2H4(ℓ) + 2H2O2(ℓ) --- N2(g) + 4H2O(g). Which is the limiting reactant in this reaction when 14.2 mol of N2H4 are mixed with 3.9 mol of H2O2?
a. H2O2

b. N2

c. N2H4

d. H2O

Part 2). How much of the excess reactant remains unchanged? Answer in units of mol.

Part 3). How much N2 is formed? Answer in units of mol.

Part 4). How much H2O is formed? Answer in units of mol.

Question

Stoichiometry Question 2?
Part 1). Some rocket engines use a mixture of hydrazine (N2H4) and hydrogen peroxide (H2O2) as the propellant. The reaction is given by N2H4(ℓ) + 2H2O2(ℓ) ---> N2(g) + 4H2O(g). Which is the limiting reactant in this reaction when 14.2 mol of N2H4 are mixed with 3.9 mol of H2O2? 
 a. H2O2 

 b. N2 

 c. N2H4 

 d. H2O 

Part 2). How much of the excess reactant remains unchanged? Answer in units of mol. 

 Part 3). How much N2 is formed? Answer in units of mol. 


 Part 4). How much H2O is formed? Answer in units of mol.

gebooors · Answer

According to reaction equation
2 moles of H2O2 for one mole N2H2

Now, if H2O2 is 3.9 mol, how much
N2H2 is needed? Is there enough it?