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AgO2 is silver oxide. An other more common example of an oxide is iron oxide, FeO2, more commonly known as rust! Most metals are not pure in their natural states, but rather are found in an oxidized state.
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What is the balanced chemical equation for the decomposition of AgsO?
AgSO = Ag(II) + S2- + O2+ =
What is the reaction for Ag plus O2 AgO?
First we have to figure out which species is oxidized and which is reduced and balance it in acid solution. On the left side, Ag has an oxidation number of 0 (it is an uncombined element). On the right side, Ag is +1. Why? Ag = +1 + 2CN- = -2 ----------------------------- Ag(CN) ion charge = -1 Note that oxygen on the left side also has an oxidation number of 0 for the same reason as Ag. But on the right side of the equation, it has formed H2O and has a charge of -2. CN- is really a spectator ion (isn't oxidized or reduced) so we can ignore it for now. Let's balance each half-reaction. I'm using = as an arrow sign. Oxidation: Ag = Ag+ + e- (done) Reduction: O2 = H2O Put a 2 in front of H2O O2 = 2H2O to balance oxygen Put 4H+ on the left side O2 + 4H+ = 2H2O to balance hydrogen Put 4e- on the left to O2 + 4H+ + 4e- = 2H2O To add the oxidation and reduction reactions together, I need to multiply the oxidation reaction by 4 so its electrons will cancel with the four that are in the reduction reaction. Doing that you get 4Ag + O2 + 4H+ = 4Ag+ + 2H2O In alkaline solution, you find the H+ above and add an equal number of OH- to BOTH sides of the equation: The 4H+ + 4OH- give 4 H2O. 4Ag + O2 + 4H+ = 4Ag+ + 2H2O +4OH- + 4OH- --------------------------------------... 4H2O If I delete two H2O from each side I get: 4Ag + O2 + 2H2O = 4Ag+ + 4OH- Finally, I can add 2CN- to each side for this: 4Ag + O2 + 2H2O + 8CN- = 4Ag(CN)- + 4OH-
Atomic number for silver?
Ag (from Latin argentum).
Who of them has greater number of electrons Ag or Ag plus?
Ag is the element Silver. Ag has more electrons than Ag+as for the element to become positively charged through a process called oxidation in which Ag has given up an electron to another element in order to obtain a positive charge. Another way to look at it is the "+" indicates a loss of a negatively charged particle which, in this case, is an electron. Proper Half-Reaction: Ag+ + e- ---> Ag
When was BDT AG created?
BDT AG was created in 1967.
How do you balance the equation for Ag2O Ag O2?
2 Ag2O --> 4Ag + O2Start with the siplest formula's without coefficients: Ag2O --> Ag + O2first balance O for two atoms: 2 Ag2O --> Ag + O2Then balance Ag for 2x2 = 4 atoms: 2 Ag2O --> 4 Ag + O2
What is the balanced chemical equation for the decomposition of AgsO?
AgSO = Ag(II) + S2- + O2+ =
What is the balanced equation for silver chlorine silver chloride?
Silver oxide --> silver and (+) oxygenAg2O --> Ag2 + O2BALANCED =2Ag2O --> 2Ag2 + O2
What is the reaction for Ag plus O2 AgO?
First we have to figure out which species is oxidized and which is reduced and balance it in acid solution. On the left side, Ag has an oxidation number of 0 (it is an uncombined element). On the right side, Ag is +1. Why? Ag = +1 + 2CN- = -2 ----------------------------- Ag(CN) ion charge = -1 Note that oxygen on the left side also has an oxidation number of 0 for the same reason as Ag. But on the right side of the equation, it has formed H2O and has a charge of -2. CN- is really a spectator ion (isn't oxidized or reduced) so we can ignore it for now. Let's balance each half-reaction. I'm using = as an arrow sign. Oxidation: Ag = Ag+ + e- (done) Reduction: O2 = H2O Put a 2 in front of H2O O2 = 2H2O to balance oxygen Put 4H+ on the left side O2 + 4H+ = 2H2O to balance hydrogen Put 4e- on the left to O2 + 4H+ + 4e- = 2H2O To add the oxidation and reduction reactions together, I need to multiply the oxidation reaction by 4 so its electrons will cancel with the four that are in the reduction reaction. Doing that you get 4Ag + O2 + 4H+ = 4Ag+ + 2H2O In alkaline solution, you find the H+ above and add an equal number of OH- to BOTH sides of the equation: The 4H+ + 4OH- give 4 H2O. 4Ag + O2 + 4H+ = 4Ag+ + 2H2O +4OH- + 4OH- --------------------------------------... 4H2O If I delete two H2O from each side I get: 4Ag + O2 + 2H2O = 4Ag+ + 4OH- Finally, I can add 2CN- to each side for this: 4Ag + O2 + 2H2O + 8CN- = 4Ag(CN)- + 4OH-
How many grams of Ag can be formed from 5.50 grams of Ag2O in the equation 2Ag2O s 4Ag s O2 g?
Given 2Ag2O(s) --> 4Ag(s) + O2(g), and 5.50g of reactant, you get 5.5/232gmol-1 (molar mass reactant)=0.0237mol, times(2) (stoichiometric ratio)=0.0474mol Ag, times(108gmol-1) (atomic mass silver)=approx. 5.12g silver.
What would you like what type of reactions is 4 Ag plus O2 arrow 2 Ag2O?
2HgO --> 2Hg + O2 is a decomposition reaction, in which Mercury oxide is decomposed into the element mercury and oxygen gas. A decomposition reaction is one in which a more complex substance is broken down into its simpler components.
If ag plus is converted to ag has it gained or lost electrons?
Ag+ + e- --> Ag
In SAP AG what is AG?
AG is short for Aktiengesellschaft
What does the AG in Daimler AG mean?
AG = Aktiengesellschaft
How many moles of Ag contain 4.4910e23 atoms Ag?
1 mole Ag = 6.022 x 1023 atoms Ag 4.4910 x 1023 atoms Ag x 1 mole Ag/6.022 x 1023 atoms Ag = 0.7468 mole Ag
What is the meaning of Ag as used in titles such as Ag Head IT department?
Acting Head of department
In Deutsche Bank AG what does AG stands for?
AG stands for Aktiengesellschaft = stock corporation.
