The industrial production of hydriodic acid takes place by treatment of iodine with hydrazine (N2H4):2 I2 + N2H4 --> 4 HI + N2(b) How many grams of HI are produced from the reaction of 115.7 g of N2H4 with excess iodine

Verified step by step guidance

1. insert step 1: Begin by identifying the balanced chemical equation for the reaction: 2 I_2 + N_2H_4 \rightarrow 4 HI + N_2.
2. insert step 2: Calculate the molar mass of N_2H_4 (hydrazine) using the atomic masses of nitrogen and hydrogen.
3. insert step 3: Determine the number of moles of N_2H_4 by dividing the given mass (115.7 g) by the molar mass of N_2H_4.
4. insert step 4: Use the stoichiometry of the balanced equation to find the moles of HI produced. According to the equation, 1 mole of N_2H_4 produces 4 moles of HI.
5. insert step 5: Calculate the mass of HI produced by multiplying the moles of HI by the molar mass of HI.

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amount of product formed from a given amount of reactant by using mole ratios derived from the coefficients in the balanced equation.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between grams and moles, enabling the calculation of how many moles of a substance are present in a given mass, which is crucial for stoichiometric calculations.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is vital for accurately calculating the yield of products in a reaction, especially when one reactant is in excess.