To test the stoichiometry of a reaction, a student placed a copper wire into a solution of silver nitrate. The reaction is Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) The student collected and recorded the following data: Mass of Cu(s) before reaction = 25.80 g Volume of AgNO3(aq) = 200 mL Concentration of AgNO3(aq) = 0.350 mol/L What mass (in g) of copper metal remains unreacted after the reaction has finished? Express your answer with three significant digits. Do not include units! g Cu

To test the stoichiometry of a reaction, a student placed a copper wire into a solution of silver nitrate. The reaction is Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) The student collected and recorded the following data: Mass of Cu(s) before reaction = 25.80 g Volume of AgNO3(aq) = 200 mL Concentration of AgNO3(aq) = 0.350 mol/L What mass (in g) of copper metal remains unreacted after the reaction has finished? Express your answer with three significant digits. Do not include units! g Cu

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

What mass of precipitate (in g) is formed when 20.5 mL of 0.400 M Mn(NO₃)₂ reacts with 32.0 mL of 0.400 M NaOH in the following chemical reaction? Mn(NO₃)₂(aq) + 2 NaOH(aq) → Mn(OH)₂(s) + 2 NaNO₃(aq)
Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.650 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.
If 28.5 g of NaOH is added to 0.800 L of 1.00 M Zn(NO₃)₂, what mass in grams of Zn(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Zn(NO₃)₂(aq) → Zn(OH)₂ (s) + 2 NaNO₃ (aq)
Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.600 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.
If 32.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)
If 16.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction?2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq)
How many grams of Cu(OH)2 will precipitate when excess NaOH solution is added to 60.0 mL of 0.684 M CuBr2 solution? CuBr₂ (aq) + 2NaOH(aq) → Cu(OH)2 (s) + 2NaBr(aq) g
570.0 mL of 0.4820 M CaCl2 is combined with 182.0 mL of aqueous 219.40 mM LICI. What is the chloride ion (CI) concentration in the resulting solution? Assume that the volumes of the two solutions are additive. Express your answer in units of millimolarity (mM) using at least three significant figures.
A sample of iron ore is dissolved in acid, and the iron is converted to Fe2*. The sample is then titrated with 47.20 mL of 0.02240 M MnO4 solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) + 4H2O How many moles of MnO4¯ were added to the solution? Blank 1 2+ How many moles of Fe were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer Blank 4 Add your answer
What mass of precipitate (in g) is formed when 20.5 mL of 0.800 M Co(NO₃)₂ reacts with 21.0 mL of 0.800 M NaOH in the following chemical reaction? Co(NO₃)₂(aq) + 2 NaOH(aq) → Co(OH)₂(s) + 2 NaNO₃(aq)
How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 69.0 mL of 0.584 M CuCl2 solution? CuCl2(aq)+2KOH(aq) → Cu(OH)2 (s) + 2KCl(aq) g
How many grams of Cu(OH)2 will precipitate when excess Ba(OH)2 solution is added to 74.0 mL of 0.786 M CuSO4 solution? CuSO4 (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + BaSO4 (aq) g