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Ch.3 - Mass Relationships in Chemical Reactions
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 70
Capitolo 3, Problema 70

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

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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.
insert step 2: Calculate the molar mass of N_2H_4 (hydrazine) using the atomic masses of nitrogen and hydrogen.
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.
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.
insert step 5: Calculate the mass of HI produced by multiplying the moles of HI by the molar mass of HI.

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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.
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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.
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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.
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An alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide: H2S + I2 → 2 HI + S (a) How many grams of I2 are needed to react with 49.2 g of H2S?

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Nickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid: NiCO3 + H2SO4 → NiSO4 + CO2 + H2O (a) How many grams of H2SO4 are needed to react with 14.5 g of NiCO3?

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Silver metal reacts with chlorine (Cl2) to yield silver chlo-ride. If 2.00 g of Ag reacts with 0.657 g of Cl2, what is the empirical formula of silver chloride?
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An alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide:H2S + I2 → 2 HI + S (b) How many grams of HI are produced from the reaction of 95.4 g of H2S with excess I2?

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