Lead (II) Sulfate reacts with Silver Nitrate to produce_______ If 616 grams Lead (II) Sulfate reacts with 612?
Lead(II) sulphate is insoluble in water. To attempt reaction you need solutions. Silver nitrate dissolves, but not lead sulphate .. so there is no reaction. It also looks as if a bit of the question is actually missing as well.
Why does lead react with H2O2?
Not sure why. Maybe you should ask peroxide.
Does peroxide react with sulphuric acid?
Yes.It can react quite in a very exothermal manner to give Caro’s acid, and water. This is the basis of Piranha solution Read the material on that link to get a better appreciation of the chemistry, and more importantly the risks involved.key words, explosive, dangerous, don’t do at home, carry out at the smallest scale possible.
Does the reaction between copper sulphate and hydrogen peroxide need a current to drive the reaction?
I will need to know how did you set it up to know what went wrong. Also I am confused with what you are saying. Is this a cell? Is this a electroplating setup? Is this a electrolysis setup?First of all, a CuSO4/H2O2 mixture reacts spontaneously in a redox reaction. Cu2+ gets reduced to Cu. H2O2 becomes O2. The copper metal produced then also becomes a catalyst for the decomposition of H2O2.If you are trying to make a cell (unlikely, since you thought that a DC is necessary), the CuSO4 and H2O2 has to be in different containers and connected by a salt bridge.If you are trying to electroplate your electrode, you don't need H2O2. Put what you want to copper-plate at the cathode, metallic copper at the anode. Dip both into a solution of CuSO4 and you are in business. Oh ya, you also need a DC for this.If you are trying to electrolysize CuSO4, again you don't need H2O2. Just dip 2 inert electrodes into a solution of CuSO4. Switch the DC on and watch one of the electrodes get a nice new pale pink shine and the other is bubbling like some fizzy drink. (The gas evolved here is O2. The gas from fizzy drinks is CO2.)Seriously, which smart aleck told you to add H2O2?
Using cobalt(II) nitrate to decompose hydrogen peroxide?
The "decomposition" of H2O2 can go in either of two ways. Peroxide can be reduced to the -2 oxidation state in hydroxide ion or oxidized to oxygen gas. H2O2 + 2e- --> 2OH- H2O2 --> O2(g) + 2H+ + 2e- Cobalt(II) is in the lowest oxidation state for an ion, and so, the only "direction" in can go is to be oxidized to Co(III). If this occurs, then peroxide is reduced to OH-. H2O2 + 2e- --> 2OH- ..... +1.77 V Co2+ --> Co3+ + 1e- ...... -1.82 V The potential for this reaction is negative, and so the reaction is nonspontaneous, assuming that the reactants are in the standard states and in concentrations of 1M. The addition of OH- will greatly reduce the concentration of Co2+ since Co(OH)2 is insoluble in water. It's possible that the cell potential will be altered enough (according to the Nernst equation) to make the reaction spontaneous.
Iron(II) is converted to iron (III) by reaction with hydrogen peroxide. Write the balanced ionic equation?
Fe^2+(aq) + H2O2(l)=====>Fe^3+(aq) + H2O(l) Half-reaction method Fe^2+(aq)====>Fe^3+(aq) add e- to the right to balance charge Fe^2+(aq)====>Fe^3+(aq) + e- H2O2(l)====>H2O(l) Add water to the right to balance O H2O2(l)====>2H2O(l) Add H+ to the left to balance H H2O2(l) + 2H+(aq)====>2H2O(l) add e- to the left to balance charge H2O2(l) + 2H+(aq) + 2e-====>2H2O(l) half reactions are Fe^2+(aq)====>Fe^3+(aq) + e- H2O2(l) + 2H+(aq) + 2e-====>2H2O(l) multiply the first one by 2 to get rid of the e- then combine the two equations 2Fe^2+(aq) + H2O2(l) + 2H+(aq)====>2Fe^3+(aq) + 2H2O(l) Now the equations is balanced. Answer is: 2Fe^2+(aq) + H2O2(l) + 2H+(aq)====>2Fe^3+(aq) + 2H2O(l)
What happens when hydrogen peroxide is mixed with iron (III) nitrate?
What happens when hydrogen peroxide is mixed with iron (III) nitrate Hydrogen peroxide = H2O2 The charge on O = -1. The charge on the stable oxide ion = -2. The O-1 in H2O2 wants to attract and electron to become O-2 iron (III) nitrate = Fe(NO3)3 The charge on Fe = +3, which is the most stable Iron ion. SO The only reaction which can occur is shown below. 2 H2O2 → 2 H2 + O2 The Fe(NO3)3 will be a catalyst for reaction, since the Fe+3 and NO3 -1 are very stable ions.
What happens if hydrogen peroxide is mixed with potassium nitrate?
Potassium nirate is KNO3. Postassium as cation is in its peak +1 oxidation state. Nitrogen in anion is in +5 oxidation state as its peak. Peroxide is H2O2. We get used to see oxygen in -2 oxidation state , but it is different here. The structure is like H-O-O-H . Oxygen is in -1 oxidation state. That is why it called peroxide.Between two no reaction can occur. Most possibly peroxide release oxygen gas and become water.2H2O2 = O2 + 2H2OPotassium nitrate remain unchanged.
What happens when hydrogen peroxide reacts with potassium iodide?
When hydrogen peroxide is added to potassium iodide in neutral solution, the potassium iodide acts as a catalyst in the decomposition of hydrogen peroxide into water and oxygen.The reaction occurs in two stages, via an intermediate oxyiodide (OI-) ion;-H2O2 (aq) + I- (aq) --> H2O (l) + OI- (aq) H2O2 (aq) + OI- (aq) --> H2O (l) + O2 (g) + I- (aq) Since the iodide ion is not consumed by the reaction, it is classed as a catalyst.In acid solution there is a different reaction. In the presence of H+ ions, the potassium iodide is oxidised by the hydrogen peroxide into elemental iodine, and the hydrogen peroxide is reduced to water;-2KI (aq) + 2H+ (aq) + H2O2 (aq) <---> I2 (s) + 2H2O (l) + 2K+ (aq)This reaction is reversible and therefore, unless the iodine is removed from the system, an equilibrium will be reached which will depend on temperature and the initial concentrations of the reactants.
What happens when hydrogen peroxide reacts with acidified KMnO4?
You get one of those occasions where hydrogen peroxide acts as a reducing agent rather than its more usual role as an oxidant. It’s oxidised to oxygen gas, whilst the permanganate is reduced to manganese dioxide:2 KMnO4 + 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2