Part C You carefully weigh out 15.00 g of CaCO3 powder and add it to 60.75 g of HCI solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 69.60 g. The relevant equation is CACO3 (s) +2HCI(aq)→H2O(1) + CO2(g) + CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA Value Units Submit

Part C You carefully weigh out 15.00 g of CaCO3 powder and add it to 60.75 g of HCI solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 69.60 g. The relevant equation is CACO3 (s) +2HCI(aq)→H2O(1) + CO2(g) + CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA Value Units Submit

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

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq). The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container? please answer d, e and f
From the list of reactions below, pick out the combustion reactions? 1) 2C2H6(g) + 7O2 (g) → 4CO2(g) + 6H2Ol) 2) MgO(s) + CO2 (g) → MgCO3(s) 3) ZnCO3(s) → ZnO (s) + CO2 (g) 4) 2CH3OH(l) + 3O2 (g) → 2CO2(g) + 4H2O(l) a 1, 2, 3, and 4 b 3 and 4 c 2, 3, and 4 d 1, 3, and 4 e 1 and 4
A 35 mL of a Na3PO4 aqueous solution and 35 mL of a BaCl2 aqueous solution were combined to form 0.520 g of Ba3(PO4)2 precipitate. If reagent tests demonstrated that Na3PO4 was the limiting reactant in the precipitation reaction, calculate the concentration of the Na3PO4 solution.
A website promoting the use of alternative energy vehicles and hybrid technologies claims that "A typical automobile in the USA uses about 500 gal of gasoline every year, producing about 5 tons of carbon dioxide." To determine the truth of this statement, calculate how many tons of carbon dioxide are produced when 500.0 gal of gasoline are combusted. Assume that the primary ingredient in gasoline is octane, C H₁ (1), which has a density of 0.703 g · mL-¹. 18 CO₂ produced: tons
The amount of mols of hydrochloric acid in 15 mL of 6.0 M HCl(aq) is 1.80 g of cadmium reacts with 0.530 g of sulfur to produce cadmium sulfide as shown by the equation, Cd(s) + S(s) → CdS(s) Which is the limiting reactant?
3) A solution of silver nitrate (AgNO3) and then prepared by dissolving 1.26 g of salt in a volumetric flask with a capacity of 250 ml. Calculate the molarity of the solution and the number of its second moles. If you knew that the molecular weight of salt is 169.9 g mol.
Determine the mass (in grams) of Ni(CO)4 made when 5.44 g of Ni reacts with 5.46 g CO. Ni (s) + 4 CO (g) →→4 (g)
A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. CACO3 (s) → Ca0(s) + CO2 (g) A 3.043 g sample of limestone-containing material gave 1.25 g of CO2, in addition to CaO, after being heated at a high temperature. What was the mass percent of CaCO3 in the original sample?
Classify each chemical reaction: Reaction BaCO3(s)→ BaO (s) + CO₂(g) 2Mg(s) + O₂(g) → 2MgO (s) Mg(s) + ZnI₂ (aq) 1 MgI₂ (aq) + Zn (s) 2Crl₂ (aq) + 3Pb(NO3)₂(aq) → 2Cr(NO3)₂(aq) + 3Pbl₂ (s) - Type ✓ choose one combination decomposition single substitution metathesis none of the above choose one X 3 C
A 1.13 g sample of an unknown bromide salt is dissolved in water. An excess of AgN 3(aq) is added, producing 1.86 g of AgBr(s) precipitate. What is the mass % of Br in the unknown salt? What is the identity of the unknown salt? You can assume the cation is from Group I or Group II.
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) → 2MnO₂ (s) + 2 CO₂ (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3MnO₂ (s) + 4A1(s) 3 Mn(s) + 2 Al₂O3(s) - Suppose the yield of the first step is 73.% and the yield of the second step is 71.%. Calculate the mass of manganese(II) carbonate required to make 8.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. do 0 x10 Ar ㅁㅁ X D G