3. Pick a "for every" statement about copper and silver in this balanced reaction. 29 47 Cu Ag Сорper 63.55 Silver 107.87 Hint: The correct balanced equation is Cu + 2A9NO, → 2Ag + Cu(NO3)2 For every 1 mole of copper, the reaction makes 2 moles of silver. For every 1 mole of copper, the reaction uses up 2 moles of silver. For every 1 mole of copper, the reaction makes 1 mole of silver. Submit Answer 3/3 submissions remaining Score:

3. Pick a "for every" statement about copper and silver in this balanced reaction. 29 47 Cu Ag Сорper 63.55 Silver 107.87 Hint: The correct balanced equation is Cu + 2A9NO, → 2Ag + Cu(NO3)2 For every 1 mole of copper, the reaction makes 2 moles of silver. For every 1 mole of copper, the reaction uses up 2 moles of silver. For every 1 mole of copper, the reaction makes 1 mole of silver. Submit Answer 3/3 submissions remaining Score:

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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For the reaction, compute the theoretical yield of the product in moles for each of the following initial reactants. Ti (s) + 2 Cl2 (g) - TiCl4(s) Express your answers using two significant figures. a) 2 mol Ti; 2 mol Cl2 b) 5 mol Ti; 9 mol Cl2 C) 0.483 mol Ti; 0.911 mol Cl2 d) 12.4 mol Ti; 15.8 mol Cl2
0.529 47.629 1. Initial mass of copper 2. Mass of copper and evaporating dish 3. Mass of evaporating dish 4. Mass of recovered copper 5. Percent yield (show cafcuntions) 6. Describe the reaction Cu(s)+HNO3(aq)→. 7. Describe the reaction Cu(NO3)2(aq)+NaOH(aq)→. 8. Describe the reaction Cu(OH)2(s)-A. 9. What are you removing by this washing? 10. What copper compound is present in the beaker? 11. Describe the reaction CuSO4(aq)+Zn(s) or CuSO4(aq)+ AI(s). 12. What is present in solution? 13. What is the gas? 14. How do you know? 15. What are you removing by washing? 16. What color is your copper sample? 17. Is it uniform in appearance? 18. Suggest possible sources of error in this experiment.
ABS plastic is a polymer consisting of three monomer units: acrylonitrile (C₃H₃N), butadiene (C₄H₆), and styrene (C₈H₈). A sample of ABS plastic contains 13.7% N by mass. It took 1.56 g of Br₂ to react completely with a 2.00 g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene units in the polymer and nothing else, so bromination is a method for determining the quantity of butadiene in the polymer. What is the percent by mass of styrene in the polymer?
3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite. involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MNCO,(s)-0,(g)→2 MnO,(s)-2 C0 (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO, (s)- 4 Al(s)-3 Mn(s)–2 Al,O,(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.
ABS plastic is a polymer consisting of three monomer units: acrylonitrile (C₃H₃N), butadiene (C₄H₆), and styrene (C₈H₈). A sample of ABS plastic contains 11.9% N by mass. It took 1.56 g of Br₂ to react completely with a 2.00 g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene units in the polymer and nothing else, so bromination is a method for determining the quantity of butadiene in the polymer. What is the percent by mass of styrene in the polymer?
Consider the following unbalanced chemical equation: MgS (s) + O2 (g) → MgO (aq) + SO2 (g) What will be the coefficient in front of O2 in the balanced chemical equation? If there is no coefficient in front of O2 in the balanced equation, please enter 1 as the answer.
Elemental iron is produced according to the following reaction: Fe2O3(s) + Al(s) ---> Al2O3(s) + Fe(s) If 5.34 g Fe2O3 is allowed to react with excess Al, what is the theoretical yield of elemental iron for this reaction? A) 0.934 g B) 1.87 g C) 3.73 g D) 6.82 g
12 Consider the following particulate-level representation. The larger spheres represent N, and the smaller spheres represent H. Which of the following statement correctly characterizes this representation? O The reactant could be represented as NH3. O The products of the reaction are N₂ and H₂. O The equation is "balanced." O If the equation for the reaction were written as shown above the coefficient of the nitrogen- containing product would be 4. O All of these statement correctly characterize this reaction.
Balance the chemical equation shown below. What is the coefficient that should be placed in front of sodium iodide (Nal)? * 1 pol Nal + Pb(SO4)2 → Pbl4 +_ Na2S04 Choose What is the coefficient that should be placed in front of lead (II) sulfate (Pb(SO4)2)? * 1 po
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5. Using the chemical equation: COg) + 2 H2(g) → CH3OH) a. Starting with 12.5 g H2 and 74.1 g CO, which is limiting reactant? b. What mass of methanol can be obtained (in theory)? c. What mass of the excess reactant is left over?