Answered: 4. What is the difference between…

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

Related questions

Question

4. What is the difference between actual yield and theoretical yield?

A) Actual yield has to do only with the reactants of a reaction, and theoretical yield has to do only with the products of a reaction.

B) Actual yield is how much is actually produced in a reaction (it has to be given or measured), and theoretical yield is a calculation that has to be done.

C) Actual yield is how much the reaction produces, and theoretical yield is how much a reaction consumes.

D) Actual yield has to do with how much you can actually get out of a reaction, and theoretical yield is how much you can get out of a reaction if you have maximum starting materials.

5. 200.0 mL of a 0.900 M solution of KCl is diluted to 600.0 mL. What is the new concentration of the solution?

6. A student combined 37.2 mL of 1.69 M KMnO₄ solution with 15.70 mL of a 0.891 M KMnO₄ solution. Calculate the concentration of the final solution.

7. How many moles of CH₃OH are there in 150.0 mL of 0.495 M CH₃OH?

8. What is the concentration of lithium ions in 0.110 M Li₂HPO₄?

9. How many mL of 0.200 M KBr would be required to make a 0.0625 M solution of KBr when diluted to 175.0 mL with water?

10. If 28.7 g of C₂H₅OH (MM = 46.07 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of C₂H₅OH in the resulting solution?

11. To what volume (in mL) would you need to dilute 25.0 mL of a 1.45 M solution of KCl to make a 0.0375 M solution of KCl?

12. Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.500 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.

13. How many moles of precipitate will be formed when 45.3 mL of 0.450 M AgNO₃ is reacted with excess MgCl₂ in the following chemical reaction? 2 AgNO₃(aq) + MgCl₂(aq) → 2 AgCl(s) + Mg(NO₃)₂(aq)

14. 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)

15. What mass of aluminum (in g) would be required to completely react with 1.95 L of 0.450 M HBr in the following chemical reaction? 2 Al(s) + 6 HBr(aq) → 2 AlBr₃ (aq) + 3 H₂(g)

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 10 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions