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. m the production of Zinc sulfide, 36 8 a of zinc is made to react with 19.4 g of sulfur. Zn +S ZnS How many moles of ZnS are produced when sulfur is completely used up? . How many grams of ZnS are produced when zinc is completely used up? C. Which reactant is the limiting reagent? How ngont are left?

. m the production of Zinc sulfide, 36 8 a of zinc is made to react with 19.4 g of sulfur. Zn +S ZnS How many moles of ZnS are produced when sulfur is completely used up? . How many grams of ZnS are produced when zinc is completely used up? C. Which reactant is the limiting reagent? How ngont are left?

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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n die production of Zinc sulfide, 36.8a of zinc is made to react with 19.4 g of sulfur. Zn +SZNS How many moles of ZnS are produced when sulfur is completely used up? . How many grams of ZnS are produced when zinc is completely used up? C. Which reactant is the limiting reagent? d. How many grams of the excess reagent are left? 2. An aqueous solution of NaOH can dissolve an aluminum sheet in the reaction: 2 Al +2 NAOH +2H20 → 2 NaAlO2 +3 H2 If 126.4 g of NaOH is 97.7 g of Al are made to react, a. How many moles of NaAIO2 are produced if 126.4 g of NaOH reacts completely? b. How many grams of NAAIO2 are produced using the same amount of NaOH? C. Which reactant is the limiting reagent? d. How many grams of the excess reagent is left? 3. Ferric chloride, FeCl3, reacts with silver nitrate, AGNO3 to form ferric nitrate, Fe(NO3)3 and silver chloride, AgCl. a. Write the balanced chemical equation of the reaction. b. If 108.5 moles of FeCl3 is combined with 76.8 moles of AGNO3, how many moles of AgCl is produced? c. How many grams of AgCl is produced? d. Which reactant is the limiting reagent? e. Which reactant is the excess reagent? BO KOM AOntpo
Transcribed Image Text:n die production of Zinc sulfide, 36.8a of zinc is made to react with 19.4 g of sulfur. Zn +SZNS How many moles of ZnS are produced when sulfur is completely used up? . How many grams of ZnS are produced when zinc is completely used up? C. Which reactant is the limiting reagent? d. How many grams of the excess reagent are left? 2. An aqueous solution of NaOH can dissolve an aluminum sheet in the reaction: 2 Al +2 NAOH +2H20 → 2 NaAlO2 +3 H2 If 126.4 g of NaOH is 97.7 g of Al are made to react, a. How many moles of NaAIO2 are produced if 126.4 g of NaOH reacts completely? b. How many grams of NAAIO2 are produced using the same amount of NaOH? C. Which reactant is the limiting reagent? d. How many grams of the excess reagent is left? 3. Ferric chloride, FeCl3, reacts with silver nitrate, AGNO3 to form ferric nitrate, Fe(NO3)3 and silver chloride, AgCl. a. Write the balanced chemical equation of the reaction. b. If 108.5 moles of FeCl3 is combined with 76.8 moles of AGNO3, how many moles of AgCl is produced? c. How many grams of AgCl is produced? d. Which reactant is the limiting reagent? e. Which reactant is the excess reagent? BO KOM AOntpo
Stoic in Action! Direction: Use a separate sheet to show your computation for the following problems: 1. Rust, Fe2O3, form from the reaction of iron and oxygen in the following equation: Fe(s)+ 02(g) → Fe,03(s) (Molar mass: Fe:55.9, O:16) a. Write the balanced equation of the reaction. b. What is the mole-mole ratio of Fe to Fe203? C. How many moles of Fe2O3 are produced from 39.4 moles of Fe? d. What is the molar mass of Fe203? e. How many grams of O2 are needed to produce 29.8 g of Fe203? 2. Given the decomposition reaction: 2 KC103(s) → 2 KCI(s) + 3 02 (g) (Molar mass: K:39.1, Cl:35.5, 0:16) a. What is the mole-mole ratio of KCIO3 to 02? b. What is the molar mass of KCIO3? c. How many moles of KCIO3 are needed to produce 36.6 moles of O2? d. How many grams of KCI are produced from an initial mass of 568.4 g KCIO3?
Transcribed Image Text:Stoic in Action! Direction: Use a separate sheet to show your computation for the following problems: 1. Rust, Fe2O3, form from the reaction of iron and oxygen in the following equation: Fe(s)+ 02(g) → Fe,03(s) (Molar mass: Fe:55.9, O:16) a. Write the balanced equation of the reaction. b. What is the mole-mole ratio of Fe to Fe203? C. How many moles of Fe2O3 are produced from 39.4 moles of Fe? d. What is the molar mass of Fe203? e. How many grams of O2 are needed to produce 29.8 g of Fe203? 2. Given the decomposition reaction: 2 KC103(s) → 2 KCI(s) + 3 02 (g) (Molar mass: K:39.1, Cl:35.5, 0:16) a. What is the mole-mole ratio of KCIO3 to 02? b. What is the molar mass of KCIO3? c. How many moles of KCIO3 are needed to produce 36.6 moles of O2? d. How many grams of KCI are produced from an initial mass of 568.4 g KCIO3?
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