Calcium carbonate reacts with hydrochloric acid solution according to the reaction below: CaCO3(s) + 2HCI (aq) → + CO2(g) CaCl2 (aq)+ H,0(1) Find the percent yield of CO2 if 22.8 g is collected when 142.2 g of CaCO3 reacts. The operation to find the number of moles of CaCO3 is: The theoretical yield of CO2 in grams is: yield =

Calcium carbonate reacts with hydrochloric acid solution according to the reaction below: CaCO3(s) + 2HCI (aq) → + CO2(g) CaCl2 (aq)+ H,0(1) Find the percent yield of CO2 if 22.8 g is collected when 142.2 g of CaCO3 reacts. The operation to find the number of moles of CaCO3 is: The theoretical yield of CO2 in grams is: yield =

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...

See similar textbooks

Similar questions

2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.
How many moles of chlorine gas react when 320.5 grams of aluminum chloride is formed? 2Al (s) + 3Cl2 (g) --> 2AlCl3 (s) (balanced)
peact Baking soda is often included in recipes to make food rise. When heated, it will produce sodium carbonate, water vapor, and carbon dioxide. Which of the five types of chemical reactions does the equation represent? Provide evidence and reasoning
For the following reaction, 3.37 grams of hydrogen gas are mixed with excess ethylene (C₂H4). The reaction yields 44.1 grams of ethane (C₂H6). hydrogen (g) + ethylene (C₂H4) (g). →→→→ethane (C₂H6) (g) What is the theoretical yield of ethane (C₂H6) ? What is the percent yield for this reaction ? Submit Answer % grams Retry Entire Group 2 more group attempts remaining
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 1. 0.0558 molO2, v=?molCO2 2. 0.0558 molO2, v= ?molH2O
For the following unbalanced reaction, suppose exactly 5.85 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. CaC₂ (s) + H₂O(1) → Ca(OH)2 (s) + C₂H₂ (9) Limiting reactant: Mass of excess reagent =
For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts. 2N2O5(g)→4NO2(g)+O2(g) - 1.2 molN2O5 Express your answer using two significant figures. -6.0 molN2O5 Express your answer using two significant figures. - 4.73×10^3 molN2O5 Express your answer using three significant figures -1.008×10−3molN2O5 Express your answer using four significant figures.
For the following reaction, 5.82 grams of water are mixed with excess chlorine gas. The reaction yields 14.0 grams of hydrochloric acid. chlorine (g) + water (1) →→→hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the theoretical yield of hydrochloric acid ? What is the percent yield of hydrochloric acid ? grams %
Ca(OH)2 (s) + H₂S(g) →→→ CaS (s) + 2H₂O(l) In the reaction above, calcium hydroxide and hydrogen sulfide react to form calcium sulfide and water. If you combine 11 g of hydrogen sulfide with 15 g of calcium hydroxide: 1) Which reactant is limiting? [Select] 2) Calculate the number of moles of calcium sulfide produced if the percent yield is 100%. [Select] ✓ mol Cas
For the following reaction, 25.3 grams of sulfur dioxide are allowed to react with 5.89 grams of water. sulfur dioxide (g) + water (1) → sulfurous acid (H₂SO3) (g) What is the maximum amount of sulfurous acid (H₂SO3) that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
[References] Use the References to access important values if needed for this question. For the following reaction, 27.8 grams of sodium chloride are allowed to react with 66.9 grams of silver nitrate. sodium chloride ( aq ) + silver nitrate ( aq) → silver chloride ( s) + sodium nitrate ( aq ) What is the maximum amount of silver chloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Visited Submit Answer Try Another Version 1 item attempt remaining Show Hint
Zinc reacts with copper sulfate in a single replacement reaction as follows Zn (s) + CuSO4 (aq) ---------------> ZnSO4 (aq) + Cu (s) If 50 grams of zinc metal were added to excess copper sulfate dissolved in a water solution, what is the theoretical yield of Cu? If 42.50 grams of copper were recovered, calculate the % yield of copper in this experiment.