1.2.3.Chemical Transformations of CopperPRESTUDYts) Balance all of the chemical reactions performed in this lab.a. Cu (s) + HNO₂ (aq) → Cu(NO₂)2 (aq) + NO₂ (g) + H₂O (1)b. Cu(NO₂)2 (aq) + NaOH (aq) → Cu(OH), (s) + NaNO, (aq)c. Cu(OH)₂ (s) → CuO (s) + H₂O (1)d. CuO (s) + H₂SO4 (aq) → CuSO. (aq) + H₂O (1)e. CuSO. (aq) + Zn (s) → Cu (s) + ZnSO₂ (aq)) Classify the reactions b, c, and e from above.A student performs the experiment detailed in this lab. The student starts with 0.085 g ofcopper wire. Referring to the balanced chemical equations in question one and applyingstoichiometric princples, answer the following questions. For full credit show a clear, concise set-up and calculation.a. How many moles of copper wire does the student have?b. How many moles of copper(II) nitrate will the student produce?c. How many moles of copper(II) hydroxide will the student produce?d. How many moles of copper(II)oxide will the student produce? YOUT23RAe. How any moles of copper(II) sulfate will the student produce?(WEN)f. How many moles of zinc metal does the student need to react completely with thecopper(II) sulfate?(60) 020 € (pol.g. How many grams of zinc metal does the student need to react completely with thecopper(II) sulfate?

We have to balance all of the chemical reactions performed in this lab:So to balance these chemical…

Answered: 1. ts) Balance all of the chemical…

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...

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Balance the reactions: CaCl2 (aq) + Na3PO4 (aq) -> NacI (aq) Ca3(PO4)2 (s) + BaCl2 (aq) + NazSO4 (aq) -> NacI (aq) + BaSO4 (s) FeCl3 (aq) + KSCN (aq) -> Fe(SCN)3 (aq) + KCI (aq)
Write the net ionic equation for the following molecular equation. 3Ca(NO3)2(aq) + 2Na3PO4(aq) → Ca3(PO4)2 (s) + 6NaNO3(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
K2SO4 (aq) + 2 H20 () 3. For which reaction will AH and AE be exactly equal to each other? 2 (g) →3 CO2 (g) + 3 H2O (g) B) 2 KOH (aq) + H2SO4 (aq) → K2SO4 (aq) + 2 H2O (1) A) C3H60 (1) +4 02 || C) N2 (g) + O2 (g) → 2 NO (2) + 02 D) 2 H2 (g) + O2 (g) →2 H20 (g) (8) E) None of the above + 02 24.02 + 4.04
3. Zinc reacts with acids according to the following equation; Zn(s) + 2HA(aq) → Zn(A),(aq) + H,(g) The net ionic reaction is; Zn(s) + 2H,O*(aq) → Zn2*(aq) + H,(g) Hydrochloric acid is a strong acid and acetic acid is a weak acid. Based on the above information, explain the difference in the two reaction rates.
Which one of the following is correct? O a. 2H20(8)→02(g) + 4H*(aq) + 4e redox reaction O b. Cr,0,2 (aq) + 20H¯(aq) → 2Cro,2 (aq) + H2O(t) redox reaction O c. NH3(g) + HCI(g) → NH4CI(s) precipitation reaction O d. 2H202-2H,0(t) + O2(g) redox reaction O e. NH3(aq) + HCI(aq) → NH4CI(aq) neutralization reaction
Fe"(aq) + OH (aq) 2. Metals in Water Write the products (except for letter d) and balance the chemical equation. Write NR on the products side if there is no reaction. a. Mg(s) + H201) → b. Zn(s) + H2O() → C. Cu(s) + H20(1) → d. Fe(s) + H2O(g) → FeO(s) + H2(9) Fe2* (aq) + OH(aq) + e- → Fe(OH)3(aq)
Classify each chemical reaction: reaction CH, OCH (1) +30₂(g) → 2CO₂ (g) + 3H₂O(g) HI (aq)+ NaOH (aq) → Nal (aq) + + H₂O(1) Mgl, (aq) + Pb(NO₂)₂ (aq) → Mg(NO3)₂(aq) + Pbl₂(s) 2 Mg(s) + F₂ (g) → 2MgF (s) - type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X O precipitation combustion acid-base O precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base S
3. A sample of KHP, KHCaH.O, weighing 2.035 g is titrated with NaOH and backtitrated with HCI. NaOH required 23.20 ml: HCl required 2.675 ml. If each ml of HCl is equivalent (*) to 0.01600 g of Na:O, what volume of 6.00 N NaOH must be addedi to 500 mL of above NaOH to bring it to 0.5000N?
III The following chemical reaction takes place in aqueous solution: 2 FeBr,(aq)+3 (NH), S(aq) Fe,S,(s)+ 6 NH, Br(aq) Write the net ionic equation for this reaction. O Chemical Reactions Writing net ionic equations ローロ G 0/3
Ff.71.
Can you answer both, parts a and b as thoroughly as possible, please? Thank you.
F2 (g) + Ga(s) → Ga (aq) + F (aq) a. F2 (g) + Ga(s) Ga+ (ag) + F(aq) b. O2 (9) + H2O(1) +Pb(s) → Pb(OH)2 (s) O2(g) + H2O(1) + Pb(s) |Pb(OH)2(s) 3+ H* (aq) + MnO4 (ag) + Fe (ag) → Mn²+ (aq) + Fe* (ag) + H2O(1) с. H (aq) + MnO4 (aq) + Fe?+ (aq) Mn2+ (aq) + Fe+ (aq) + H2O(1)

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