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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 HALF reaction between I2 and S2O3?
In the redox reaction between iodine (I₂) and thiosulfate (S₂O₃²⁻), the half-reaction for iodine is the reduction of I₂ to iodide (I⁻). The half-reaction can be represented as: [ \text{I}_2 + 2 \text{e}^- \rightarrow 2 \text{I}^- ] For thiosulfate, it acts as a reducing agent and is oxidized to sulfate (SO₄²⁻), but the focus here is on the reduction of iodine.
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.
What type of process is the balanced half-reaction in which chlorine gas is reduced to the aqueous chloride ion is?
The balanced half-reaction in which chlorine gas (Cl₂) is reduced to the aqueous chloride ion (Cl⁻) is an electrochemical reduction process. In this reaction, chlorine gas gains electrons, resulting in the formation of chloride ions. This process typically occurs in an electrolytic or galvanic cell, where it plays a crucial role in redox reactions. The overall half-reaction can be represented as: Cl₂ + 2e⁻ → 2Cl⁻.
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 is the reaction half reaction for Mg plus O2 2Mgo?
The reaction of magnesium (Mg) with oxygen (O₂) to form magnesium oxide (MgO) can be represented by the half-reactions for each element. For magnesium, the oxidation half-reaction is: [ \text{Mg} \rightarrow \text{Mg}^{2+} + 2e^- ] For oxygen, the reduction half-reaction is: [ \text{O}_2 + 4e^- + 2\text{H}_2O \rightarrow 4\text{OH}^- ] Combining these half-reactions, you ultimately get the overall balanced reaction: [ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} ]
What occurs at the cathode of a galvanic cell?
An oxidation half-reaction
