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2 Ag2O --> 4Ag + O2
- Start with the siplest formula's without coefficients: Ag2O --> Ag + O2
- first balance O for two atoms: 2 Ag2O --> Ag + O2
- Then balance Ag for 2x2 = 4 atoms: 2 Ag2O --> 4 Ag + O2
Wiki User
∙ 12y ago
Wiki User
∙ 15y ago2Ag2O ----> 4Ag + O2 Silver oxide ---> silver + oxygen
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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.
How do you balance 2H2 O2 2H2O O2?
2H2O2 ==> 2H2O + O2 the equation is balanced
How do you balance this equation C plus O2---CO?
2c + o2---2co
How do i insert the coefficients to balance the equation SO2 plus O2 SO3?
The chemical equation is:2 SO2 + O2 = 2 SO3
How do you balance the equation Al plus O2 yields Fe2O3?
Al + O2 will never yield Fe2O3.
What is the Combustion of silver oxide?
Decomposes into metallic silver and oxygen.
What does the reaction between iron and silver oxide make and what is the balanced equation showing this?
Because Ag2O (as oxidator) is more reactive than FeO, so Fe (as reductor) can abstract the oxide O (O2-) from Ag2O according to electrochemical series (which says: Ag is less reactive to oxygen than Fe, Ag is a more 'noble' metal)Fe + Ag2O --> FeO + 2Ag
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-
What is the balanced equation for silver chlorine silver chloride?
Silver oxide --> silver and (+) oxygenAg2O --> Ag2 + O2BALANCED =2Ag2O --> 2Ag2 + O2
If 2Ag2O and 4Ag o2 then if you started with 3.25 moles of Ag2O how many moles of O2 would be produced?
what is ag2o
What is the balance equation for N2 and O2?
N2 + o2 = no2
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.
How do you balance the equation for H2 plus O2 H2O?
This simple equation is: 2H2 + O2 = 2H2O
How do you balance 2H2 O2 2H2O O2?
2H2O2 ==> 2H2O + O2 the equation is balanced
How do you balance this equation C plus O2---CO?
2c + o2---2co
What is the balanced chemical equation for the decomposition of AgsO?
AgSO = Ag(II) + S2- + O2+ =
How do i insert the coefficients to balance the equation SO2 plus O2 SO3?
The chemical equation is:2 SO2 + O2 = 2 SO3
