Directions: Make sure you show your work (calculations) in all of these stoichiometry problems. 1. If 20.0 grams of Sodium hydroxide reacts with 30.0 grams of Sulfuric acid to produce Sodium sulfate and water, which reactant is the limiting reactant? 2. If 40.0 grams of phosphoric acid reacts with 60.0 grams of magnesium carbonate in a reaction, the products are magnesium phosphate, carbon dioxide and water. A) Write a balanced chemical equation. B) Determine the Limiting Reactant. C) How many grams of magnesium phosphate are produced? D) How many grams of water are produced? 3. If 20.0 grams of Potassium hydroxide reacts with 15.0 grams of Ammonium sulfate in a double replacement reaction. The products are Ammonia, NH3, Water, and Potassium sulfate (a) Determine the Limiting Reactant and then calculate the: (b) moles of Potassium sulfate produced (c)grams of Ammonia, NH3 produced

Directions: Make sure you show your work (calculations) in all of these stoichiometry problems. 1. If 20.0 grams of Sodium hydroxide reacts with 30.0 grams of Sulfuric acid to produce Sodium sulfate and water, which reactant is the limiting reactant? 2. If 40.0 grams of phosphoric acid reacts with 60.0 grams of magnesium carbonate in a reaction, the products are magnesium phosphate, carbon dioxide and water. A) Write a balanced chemical equation. B) Determine the Limiting Reactant. C) How many grams of magnesium phosphate are produced? D) How many grams of water are produced? 3. If 20.0 grams of Potassium hydroxide reacts with 15.0 grams of Ammonium sulfate in a double replacement reaction. The products are Ammonia, NH3, Water, and Potassium sulfate (a) Determine the Limiting Reactant and then calculate the: (b) moles of Potassium sulfate produced (c)grams of Ammonia, NH3 produced

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter10: Quantity Relationships In Chemical Reactions

Section: Chapter Questions

Problem 70E: Classify each of the following statements as true or false: a Coefficients in a chemical equation...

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Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
The reaction of ethylene oxide with water to give ethylene glycol (automobile antifreeze) occurs in 96% actual yield. How many grams of ethylene glycol are formed by reaction of 35.0 g of ethylene oxide? in case the following picture of chemical reaction does not show up in your computer, here is the chemical equation: Ethylene Oxide (C2H4O) + H2O ⟶⟶ Ethylene glycol (C2H6O2)
1. 1.95 g H2 is allowed to react with 10.5 g N2, producing 2.29 g NH3, according to the unbalanced equation. H2 (g) + N2 (g) → NH3 (g) What is the percent yield for this reaction? Solve: 1) Record and list every NUMBER with UNIT AND ENTITY (As Given); Label them as either reactant or product if an equation is given. Write down Desired UNIT AND ENTITY. Given: 1.95 ____ _________; Reactant or Product (Circle one) 10.5 ____ _________; Reactant or Product (Circle one) 2.29 ____ __________; Reactant or Product (Circle one) Desired: percent yield of _________
a. For the following unbalanced chemical equation, suppose exactly 4.45 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. Na + Br2 = NaBr Limiting Reactant: ? Mass of NaBr: ?
For the reaction of sodium sulfide with iron(III) chloride below (as an unbalanced reaction - that's how I will almost always give you reactions. ALWAYS check to see if a reaction is balanced before you use it. You balanced it in the last question; make sure you have that right before you start calculating!), you have 319.5 kg of sodium sulfide and 502.3 kg of iron(III) chloride available. What mass (in kilograms) of sodium sulfide do you NEED if you're going to reduce all of the iron(III) chloride you have? Na2S(s) + FeCl3(s) → Fe2S3(s) + NaCl(s)
In our bodies, sugar is broken down with oxygen to produce water and carbon dioxide. For the following reaction, 0.597 moles of glucose () are mixed with 0.160 moles of oxygen gas. glucose (C6H12O6)(s) + oxygen(g)-----> carbon dioxide(g) + water (l) What is the formula for the limiting reagent? _______ What is the maximum amount of carbon dioxide that can be produced? ________ moles
How many grams of solid copper will theoretically be produced when 14.4g of aluminum is reacted with 14.4g of copper (II) sulfate? Which reactant is the limiting reactant? Show work. Be sure to include units.
Stoichiometric calculations. (Show computations) M, a PhD student considers synthesizing ammonia using nitrogen and hydrogen. Supposed that 26 grams of N2and 20 grams of H2 are initially present. Use the chemical reaction as a guide and answer the following questions. N2 + H2 à NH3 Balance the chemical reaction. What is the MW of N2, H2, and NH3? How many moles of NH3can be produced from 26 grams of N2? How many moles of NH3can be produced from 20 grams of H2? Which reactant is the limiting reactant? How many grams of NH3will be produced from this mixture of two reactants?
2.Given the following balanced chemical equation, how many grams of NaClO3 would be produced from the reaction of 44.8 g Sodium sulfide and an excess amount of Iron (II) chlorate? Fe(ClO3)2 + Na2S --> FeS + 2NaClO3 g NaClO3 All work must be shown and submitted. Any steps left out may result in a loss of points for that particular problem.
When magnesium is heated in air, it reacts with oxygen to form magnesium oxide. suppose a piece of magnesium reacts with oxygen and the mass of the solid increases by 1.30g. How many grams of magnesium reacted? ____ g Mg not just answer but how to come to that answer
Please answer all parts. 1. Consider the balanced reaction of sodium with bromine gas to form sodium bromide. 2Na (s) + Br2 (g) --> 2NaBr (s) a. If you start with 2.5 moles of sodium and 1.5 moles of bromine, which is the limiting reactant? Show calculations please. b. If you start with 50.0 grams of sodium and 50.0 grams of bromine, calculate the limiting and excess reactant. Show calculations pelase.