   Chapter 4, Problem 64PS

Chapter
Section
Textbook Problem

Hydrazine, N2H4, a base like ammonia, can react with sulfuric add.2 N2H4(aq) + H2SO4(aq) → 2 N2H5+(aq) + SO42–(aq)What mass of hydrazine reacts with 250. mL of 0.146 M H2SO4?

Interpretation Introduction

Interpretation:

It should be determine that the mass of hydrazine, which is required to react with 250.0mlof0.146MH2SO4

Concept introduction:

Numberofmole=GivenmassofthesubstanceMolarmass

• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
Explanation

Balanced chemical equation for the given reaction is,

2N2H4(aq)+H2SO4(aq)2N2H5+(aq)+SO42(aq)

The amount (moles) of H2SO4  available can be calculated by as follows,

Before that 250.0mLH2SO4 is converted into L.

Thus amount of H2SO4 available,

0.025LH2SO4×(0.146molH2SO41LH2SO4)=0.001825molH2SO4

By using the stoichiometric factor calculating the amount of hydrazine required based on the amount of H2SO4 as follows

0

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