Question

How many moles of oxygen are needed to react with 160 g of hydrazine?

a) 1 mole
b) 2 moles
c) 3 moles
d) 4 moles

Answer 1

To determine the number of moles of oxygen needed to react with hydrazine, we can use the balanced chemical equation and the molar mass of the compounds involved.

Step-by-step explanation:

To determine how many moles of oxygen are needed to react with 160 g of hydrazine, we need to first write the balanced chemical equation for the reaction. The balanced equation is:

N2H4 + O2 → N2 + 2H2O

We can see that 1 mole of hydrazine (N2H4) reacts with 1 mole of oxygen (O2) to produce 2 moles of water (H2O). Since hydrazine has a molar mass of 32 g/mol and oxygen has a molar mass of 32 g/mol, the number of moles of oxygen needed can be calculated as follows:

160 g hydrazine × (1 mol hydrazine / 32 g hydrazine) × (1 mol oxygen / 1 mol hydrazine) = 5 moles of oxygen

Therefore, the correct answer is c) 3 moles.