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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use the References to access important values if needed for this question. For the following reaction, 26.8 grams of sulfur dioxide are allowed to react with 6.14 grams of water. sulfur dioxide(g) + water (1)→ sulfurous acid (H₂SO3)(g) What is the maximum mass of sulfurous acid (H₂SO3) that can be formed? g What is the FORMULA for the limiting reactant? Mass= What mass of the excess reagent remains after the reaction is complete? Mass= Submit Answer b.0 g Retry Entire Group Show Hint 8 more group attempts remaining Previous Next> Save and Exit
3. Table salt (NaCl) is produced when sodium element reacts with chlorine gas. a) Write the balance chemical reaction. 2 Na +Cl2 2nacI b) Determine the mass of NaCl produced when 12.8 g of sodium reacts. c) Determine the mass of NaCl produced with 10.2 g of chlorine gas reacts. d) Which amount, 12.8 g of sodium or 10.2 g of chlorine gas, provides a better yield of NaCI?
Relate the model to Chemistry: The balanced chemical reaction for producing water is: 2 H2 + 1 O2 → 2 H2O. Predict which reactant amounts (of the three examples shown below) would get the most water with the least amount of leftovers. Explain how your understanding of Limiting Reactant helped you figure this out.
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Alkali metal hydroxides are sometimes used to "scrub" excess carbon dioxide from the air in closed spaces (like submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide according to the following unbalanced chemical equation: Suppose a lithium hydroxide canister contains 180. g of . What mass of will the canister be able to absorb? Mass = g If it is found that after 24 hours of use the canister has absorbed 120. g of carbon dioxide, what percentage of its capacity has been reached? Percentage = %
SHOW COMPLETE SOLUTION USING STOICHIOMETRY AND BOX THE FINAL ANSWER.
Dinitrogen monoxide which is commonly called as nitrous oxide (N₂O) reacts completely with an equimolar amount of nitrogen dioxide gas. The products of the reaction are nitrogen gas and oxygen gas. The percent yield for the reaction is 76.6%. Calculate the mass of nitrogen gas (in grams) produced in the reaction from 6.09 g of N₂O. Hint: Write the balanced chemical equation. (Give 3 sig figs in your answer)
Can you please answer 1,2,3 please