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The equation AgNO3 plus Cu à CuNO3 plus Ag represents which type of reaction?
This is a displacement reaction: Copper is (barely) higher in the electromotive series than silver, so that the silver in a compound can be displaced by copper, resulting in the formation of unreacted silver.
What is the overall voltage for a redox reaction with the half reactions Ag e Ag and Cu2 2e?
0.80-0.34
What is the word equation for the reaction between copper and silver nitrate?
It would produce Silver and a blue solid called Copper Nitrate (Cu(NO3)2). It is caused by a replacement reaction where Copper replaced Silver in Copper Nitrate. The equation goes like this: Cu + Ag(NO3)2 → Ag + Cu(NO3)2
What is the oxidizing agent for Zn plus CuCl2--ZnCl2 plus Cu?
In the reaction Zn + CuCl2 → ZnCl2 + Cu, CuCl2 is the oxidizing agent because it accepts electrons from Zn, causing zinc to be oxidized and copper to be reduced.CuCl2 itself gets reduced to Cu.
What is the oxidation half reaction of Cl2 2Cu to 2CuCl?
Cl2 + 2Cu --> 2CuCl Oxidation reaction is Cu --> Cu+ + 1e Reduction reaction is Cl + 1e --> Cl- Redox reaction is Cu + Cl --> Cu+ + Cl-
In a particular reaction between copper metal and silver nitrate 12.7 g Cu produced 38.1 g Ag. What is the percent yield of silver in this reaction Cu plus 2AgNO3 and acirc and 134 and 146 Cu(NO3)2 pl?
To calculate the percent yield of silver (Ag) in the reaction, we first need to determine the theoretical yield of Ag based on the amount of Cu used. The balanced chemical equation shows that 1 mole of Cu produces 2 moles of Ag. The molar mass of Cu is approximately 63.55 g/mol, and that of Ag is about 107.87 g/mol. From 12.7 g of Cu, we can calculate the moles of Cu: [ \text{Moles of Cu} = \frac{12.7 \text{ g}}{63.55 \text{ g/mol}} \approx 0.199 \text{ moles} ] Since 1 mole of Cu produces 2 moles of Ag, the theoretical yield of Ag would be: [ 0.199 \text{ moles Cu} \times 2 \text{ moles Ag/mole Cu} \times 107.87 \text{ g/mol} \approx 43.0 \text{ g Ag} ] Now, using the actual yield of 38.1 g Ag, the percent yield can be calculated as: [ \text{Percent Yield} = \left(\frac{38.1 \text{ g}}{43.0 \text{ g}}\right) \times 100 \approx 88.8% ] Thus, the percent yield of silver in this reaction is approximately 88.8%.
What is the balanced formula for cooper metal plus silver nitrate solution yield silver plus copper II nitrate solution?
The reaction is:Cu + 2 AgNO3 = Cu(NO3)2 + 2 Ag
Single replacement of cu plus AgNO3?
Cu + AgNO3 → Ag + Cu(NO3)2 In this reaction, copper (Cu) is more reactive than silver (Ag), so it will replace silver in the compound AgNO3, resulting in the formation of silver metal and copper nitrate.
If silver and copper are used to make a cell what half-reactions will occur for ag plus aq plus e- ag s e0 equals 0.80 v and for cu2 plus aq plus 2e- cu aq e0 equals 0.34 V?
In the cell, the half-reaction for silver will be Ag+ (aq) + e- -> Ag (s) with a standard reduction potential of +0.80 V. The half-reaction for copper will be Cu2+ (aq) + 2e- -> Cu (s) with a standard reduction potential of +0.34 V. The silver half-reaction will occur at the cathode, while the copper half-reaction will occur at the anode in the cell.
Where did this substance Cu plus 2AgNO3 --- CuNO32 plus 2Ag come from?
This reaction involves the reaction of copper (Cu) with silver nitrate (AgNO3) to form copper(II) nitrate (Cu(NO3)2) and silver (Ag). It is a chemical reaction that was likely conducted in a laboratory setting or for academic purposes.
Write out this reaction in words AgNO3 plus Cu-CuNO3 plus Ag?
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The equation AgNO3 plus Cu à CuNO3 plus Ag represents which type of reaction?
This is a displacement reaction: Copper is (barely) higher in the electromotive series than silver, so that the silver in a compound can be displaced by copper, resulting in the formation of unreacted silver.
Cu and AgCl equals Ag plus CuCl2?
cu(II) + 2agcl --> 2ag+cucl2
What is the overall voltage for a redox reaction with the half reactions Ag e Ag and Cu2 2e?
0.80-0.34
Copper will react with silver nitrate to form copper nitrate and silver From this reaction 127.1 grams of copper will produce how many grams of silver?
The balanced equation for the reaction is: Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag Calculate the molar mass of Cu and Ag (Cu = 63.55 g/mol, Ag = 107.87 g/mol). Using the molar ratio of Cu to Ag (1:2), convert the mass of Cu to moles, then use the molar ratio to find the moles of Ag produced. Finally, convert moles of Ag to grams using the molar mass of Ag to find the grams of silver produced.
WHAT IS THE OVERALL VOLTAGE FOR A REDOX REACTION HE HALF REACTIONS AG plus E-ag(S) AND CU(S) CU2 plus 2E?
To determine the overall voltage for the redox reaction involving the half-reactions ( \text{Ag}^+ + e^- \rightarrow \text{Ag}(s) ) and ( \text{Cu}(s) \rightarrow \text{Cu}^{2+} + 2e^- ), we first need the standard reduction potentials. The standard reduction potential for silver (( \text{Ag}^+ )) is +0.80 V, and for copper (( \text{Cu}^{2+} )) is +0.34 V. Since silver is reduced and copper is oxidized, the overall cell potential is calculated as ( E_{\text{cell}} = E_{\text{reduction}} - E_{\text{oxidation}} = 0.80 , \text{V} - 0.34 , \text{V} = 0.46 , \text{V} ). Thus, the overall voltage for the redox reaction is +0.46 V.
What is the balanced equation between coper metal and silver solid?
There is NO reaction between Cu and Ag.
