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A limiting reagent is Choose...consumed completelyleft over in excess during a chemical reaction, and it Choose...decreasesincreases the possible amount of product that can be formed.
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A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The reaction is:
K2CO3(aq) + CaCl2(aq) = CaCO3(s) + 2KCl(aq).
Based on the masses of the two reactants given, the limiting reagent is Choose...CaCl2K2CO3 .
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Based on the data, the balanced equation, and the limiting reagent in question 2, what is theoretical yield in grams of CaCO3? Give your answer to the correct number of significant figures. Just type in the number. Do not include the units in your answer.
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Go back to the data, the balanced equation, and the limiting reagent in question 2, as well as the theoretical yield in question 3. If the actual yield of CaCO3 is 6.15 grams, what is the percent yield of the reaction? Give your answer to the correct number of significant figures. Do not include the percent (%) sign.
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If well water (containing calcium ions in addition to other minerals) is used rather than deionized water to prepare the reactant solutions, the experimental / actual yield of calcium carbonate:
Select one:
increases
decreases
stays the same
Question text A limiting reagent is Choose...consumed completelyleft over in excess during a chemical reaction, and...
Not yet answered Graded out of 1.00 Flag question Question text In the process of photosynthesis, water and carbon dioxide are produced. Select one: True False Question 2 Not yet answered Graded out of 1.00 Flag question Question text In the carbon cycle, combustion produces atmospheric oxygen. Select one: True False Question 3 Not yet answered Graded out of 1.00 Flag question Question text In a balanced chemical equation, the number of each type of atom in the reactants must...
Question 1 The following is the data you will use for this activity. Not yet answered Vol Used Points out of 2.00 3.5 mL Reactants benzonitrile sodium hydroxide (109) Product P Flag 28.6 mL question Exp % Yield benzoic acid 81.6 % Calculate the grams of benzonitrile used. Answer: Question 2 Calculate the moles of benzonitrile used. Not yet answered Points out of 2.00 Answer: Flag question Question 3 Calculate the mass of sodium hydroxide used in grams. Not yet...
reaction that has a theoretical yield of 10. In the reaction below, identify the reactants. CaCl2 (aq) + K2CO3 (aq) → CaCO3 (s) + 2 KCI (aq) Ca. CaCl2 and K2CO3 . CaCO3 and KCI c. CaCl2 and CaCO3 d. K2CO3 and KCI e. K2CO3 and CaCO3 11. Select the number of moles of CO2 formed by the reaction of 0.153 mol C3Hg with excess Oz. C3H3(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) a. 0.153 mol CO2...
Not yet answered Points out of 2 Flag question Question text 11.3 grams of ammonium chloride (NH4Cl) are dissolved in enough water to make 155 mL of solution. What is the resulting Molarity of the aqeuous solution? Give your answer to the correct number of significant figures. Type in only the numbers. Do not include the molarity unit (M or moles/L). Hint: you need to solve for the molar mass of ammonium chloride to do this calculation. Answer: Question 2...
For the balanced reaction: CaCl2 (aq) + Na2CO3 (aq) -> CaCO3 (s) + 2 NaCl (aq), calculate the moles of CaCO3 that form when 5.00 mL of 0.587 M CaCl2 (aq) reacts with 5.00 mL of 0.595 M Na2CO3 (aq). Enter your answer in the correct number of significant figures. Hint: This is limiting reactant problem.
Use the following atomic weights & quantities to calculate overall % yield of diphenylacetylene. Remember that your yield must be based on the limiting reagent, and that grams must be converted to moles. For problems not involving a one to one stoichiometry ot may be easier to calculate the theoretical yield in grams from both reagents to determine which is truly the limiting reagent. Filling out most of the chart will help. Give ONLY two significant digits in your answer....
7. What is a limiting reagent? The substance that is to when the chemical reaction that is totally hemical reaction consumed is complete. 8. How many moles of salicylic acid many moles of salicylic acid are there in 5.0 grams? Show all your work. Moles = x grams=5.ograma CyH603 (-128 moles 12 H6VI olor Moss 0 - 10X3 138 g/mol Moles= 5.ograme -0.0362 moles) 1389 Imolt 9. What is the mass of 10.0 mL of acetic anhydride? Show all your...
Solution Stoichiometry: The next step in the lab is to carefully measure out 25.00 mL of the 0.250 M Na2CO3 solution, and 30.00 mL of the 0.200 M CaCl2 solution, and mix them together. Use Reaction Stoichiometry to predict the limiting reactant in the reaction, and the amount in grams of calcium carbonate that we expect to precipitate (theoretical yield). Remember: M= mols solute / L solution Use the following table to help organize your information. 0.250 M Na2CO3 00.200M...
Question 1 1 pts Calculate the mass of potassium chloride, KCI, (in grams) formed when 7.00 g of chlorine gas is allowed to react with 5.00 g of potassium. (write the chemical reaction first) 7.36 7.38 14.7 4.77 9.53 Question 2 1 pts Carbon dioxide is produced in the following reaction: 5 H2C204(aq) + 2 KMnO4 (aq) + 3 H2SO4 (aq) → 10 CO2(g) + 2 MnSO4 (aq) + K2SO4 (aq) + 8 H20 (1) What is the limiting reagent...
the reaction is: CaCl2(aq) + Na2CO3(aq) ? CaCO3(s) + 2NaCl(aq) Mass Grams Mass of CaCl Mass of Na2CO Mass of Filter Paper Mass of Product, CaCO3 (Experimental Yield) Experimental Observations 2 gm 2.5 gm 2.3 gm 2.4 gm 1. What is the proper name of CaCO? When is it used in real life? 2. What happened to the excess reactant after the reaction was complete? 3. What was the limiting reagent in your experiment? Show your calculations that prove this....