HomeworkLib
Question

Consider the following unbalanced equation. Starting with 0.80 g of elemental copper and 20. mL of...

Consider the following unbalanced equation. Starting with 0.80 g of elemental copper and 20. mL of 15 M nitric acid (18.9 g), _____mole of water would be produced.

Cu(s) + HNO3(aq) ---->Cu(NO3)2(aq) + NO2(g) + H2O(l)

a. 0.030 b. 0.80 c. 0.0126 d. 0.025 e. 0.0252

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
Consider the following unbalanced equation. Starting with 0.80 g of elemental copper and 20. mL of...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Write a balanced equation for the reaction of copper with nitric acxid tp produce nitric oxide...

    Write a balanced equation for the reaction of copper with nitric acxid tp produce nitric oxide (NO). Predict whether this reaction would occur with more, or less concentrated nitric acid than equation (1) : Cu(s) + HNO3(aq) ---> Cu(NO3)2(aq) + NO2(g) +H2O(l)

  • Concentrated nitric acid reacts with solid copper to give nitrogen dioxide gas and dissolved copper ions...

    Concentrated nitric acid reacts with solid copper to give nitrogen dioxide gas and dissolved copper ions according to the equation: Cu(s) + 4 H+(aq) + 2 NO3 - (aq) → 2 NO2(g) + Cu2+(aq) + 2 H2O(l) Suppose that 6.80 g of copper is consumed in this reaction and that the NO2 is collected at a pressure of 0.970 atm and a temperature of 45 oC. What volume of NO2 is produced?

  • Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3...

    Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H2O(ℓ) What mass of NO(g) can be formed when 20.7 g of Cu reacts with 50.0 g HNO3?           g NO

  • 1. Balance the three copper reactions: + H20 (1) Cu(NO3)2 (aq) + NO2(g) i) Cu (s)...

    1. Balance the three copper reactions: + H20 (1) Cu(NO3)2 (aq) + NO2(g) i) Cu (s) + HNO3 (aq) ii) Cu(NO3)2 (aq) + NaOH(aq) Cu(OH)2 (s) + NaNO3(aq) (aq) - iii) Cu(OH)2 (S) Cuo(s) + H2O (1) 2. In reaction (i), suppose you add 4.0 mL of 6 M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)

  • 1. Balance the three copper reactions: +H20 (1) +NO2 (g) Cu(NO3)2 (aq) i) Cu (s) HNO3...

    1. Balance the three copper reactions: +H20 (1) +NO2 (g) Cu(NO3)2 (aq) i) Cu (s) HNO3 (aq) NANO3 (aq) NaOH (aq) Cu(OH)2 (s) + ii) Cu(NOs)2 (aq) + H2O (1I) CuO (s) iii) Cu(OH)2 (s) 2. In reaction (i), suppose you add 4.0 mL of 6M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)

  • please answer Titration Homework 1. Copper reacts with dilute nitric acid according to the equation 3...

    please answer Titration Homework 1. Copper reacts with dilute nitric acid according to the equation 3 Cu(s) + 8 HNO, (aq) + 3 Cu(NO3)2 (aq) + 2NO(g) + 4H20 (1) If a copper penny weighs 3.020g is dissolved in a small amount of nitric acid and the resulting solution is diluted to 50.0 mL with water, what is the molarity of the Cu(NO3)?

  • 3. (14%) The metal copper is oxidized in nitric acid according to the equation: 3 Cu...

    3. (14%) The metal copper is oxidized in nitric acid according to the equation: 3 Cu + 8 HNO3 → 3 Cu (NO3) 2 + 2 NO + 4 H2O a) Show how you set the oxidation-reduction reaction and get the equation here above (show as many steps in the process) b) You receive 0.3855 g of copper-containing metal together with other dissolved substances easily set up. You find that to dissolve the copper and form copper nitrate Cu (NO3)...

  • In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate,...

    In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) +   2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...

  • In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate,...

    In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) +   2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...

  • Copper start to finish lab questions 7a.) and 7b.) hopefully the last 2 images of information...

    Copper start to finish lab questions 7a.) and 7b.) hopefully the last 2 images of information help make the problem clearer 7. a) For each mole of Cu dissolved in the nitric acid solution (HNO3), how many moles of [Cu(H2O)612+ are formed? col were formed in your reaction? b) Given your data above, how many moles of [Cu(H2O)6]2+ Reaction I:Cu (s)+ 4 H3O (aq) +2 NO3 (aq) --> [Cu(H2O)]** (aq) +2 NO2 (g) The first reaction in the series is...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT