0
What else can I help you with?
What is the balanced half equation for bromine and potassium iodide?
Br2 + (2e)- --> 2 Br- 2I- --> I2 + (2e)-
Formula for copper sulfite?
These are the ions and their charges: Cu+2 SO3-2The charges have to add up to zero, so one +2 copper ion cancels out one -2 sulfite ion. Therefore, the formula is CuSO3.
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-
Which balanced equation represents an oxidation-reduction reaction?
Equations that separate the oxidation from the reduction parts of the reaction
What is the oxidation half-reaction for 2Mg O22MgO?
The oxidation half-reaction for the conversion of 2Mg to MgO is: 2Mg(s) -> 2Mg^2+(aq) + 4e^-
What is the balanced half reaction for the oxidation of hydrogen peroxide?
The balanced half reaction for the oxidation of hydrogen peroxide is: 2H2O2 - O2 2H 2e-
Is c2h6o o2 balanced?
No! Looks like half a combustion reaction and I do not mean the half reaction method. C2H6O + 3O2 -> 2CO2 + 3H2O
What is the balanced chemical equation for the reaction of zinc with dilute hydrochloric acid and equation of it's oxidation half reaction also reduction half reaction?
Balanced chemical equation: Zn (s) + 2HCl (aq) --> ZnCl2 (aq) + H2 (g) Oxidation half-reaction: Zn (s) --> Zn2+ (aq) + 2e- Reduction half-reaction: 2H+ (aq) + 2e- --> H2 (g)
What is The balanced half-reaction in which chlorine gas is reduced to the aqueous chloride ion?
The balanced half-reaction for the reduction of chlorine gas (Cl₂) to chloride ion (Cl⁻) is: Cl₂ + 2e⁻ → 2Cl⁻
What is the balanced half equation for bromine and potassium iodide?
Br2 + (2e)- --> 2 Br- 2I- --> I2 + (2e)-
What is the overall redox reaction of cr2o7 plus br?
The overall redox reaction of Cr2O7 + Br is not a balanced equation. To balance the equation, the half-reactions for the oxidation and reduction of each element need to be determined and balanced first.
How can one balance redox reactions in acidic solutions effectively?
To balance redox reactions in acidic solutions effectively, follow these steps: Write the unbalanced equation for the redox reaction. Separate the reaction into half-reactions for oxidation and reduction. Balance the atoms in each half-reaction, excluding oxygen and hydrogen. Balance the oxygen atoms by adding water molecules. Balance the hydrogen atoms by adding H ions. Balance the charges by adding electrons to one or both half-reactions. Ensure that the total charge and number of atoms are balanced in both half-reactions. Multiply each half-reaction by a factor to equalize the number of electrons transferred. Combine the balanced half-reactions to form the overall balanced redox reaction. By following these steps, one can effectively balance redox reactions in acidic solutions.
How to combine half-reactions to form a balanced redox equation?
To combine half-reactions to form a balanced redox equation, first balance the atoms in each half-reaction, then balance the charges by adding electrons. Finally, multiply the half-reactions by coefficients to ensure the number of electrons transferred is the same in both reactions.
What occurs at the cathode of a galvanic cell?
An oxidation half-reaction
What is the observation after half an hour when copper sulfate reacts with magnesium?
After half an hour, you would observe that the magnesium has started to dissolve into the copper sulfate solution, forming a blue solution due to the formation of copper ions in solution. Bubbles of hydrogen gas should also be observed as a byproduct of the reaction.
What procedure is used to convert acidic conditions to basic conditions when balancing redox half-reaction equations?
To convert acidic conditions to basic conditions when balancing redox half-reaction equations, you can add hydroxide ions (OH⁻) to both sides of the equation. First, balance the half-reaction under acidic conditions, then add the equivalent amount of OH⁻ to neutralize the hydrogen ions (H⁺) present. This results in the formation of water (H₂O), which can then be simplified to achieve the final balanced half-reaction in basic conditions.
Why only half molecule of water get loss when gypsum is heated?
When gypsum is heated, it undergoes a chemical reaction where some of the water molecules are removed to form calcium sulfate hemihydrate (plaster of Paris). This process results in the loss of only half of the water molecules originally present in gypsum, leaving one water molecule attached to the calcium sulfate to form the hemihydrate product.
