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What is the complete redox reaction for MnO4- and H2O2 under acid conditions?
2 H2O2 -- [MnO2] --> 2 H2O + O2 A catalyst does not take place in a chemical reaction, thus it cannot be placed at the reactant or product side of the reaction equation. In stead it is usually placed above the reaction arrows, sometimes between right brackets: -- [MnO2] -->
A reaction in which products can react to re-form reactants is?
A chemical reaction in which the products re-form the original reactants is called a reversible reaction.
Does a sodium atom gain one electron?
It keeps its neutrons but loses one electron. Protons and neutrons do not move in a chemical reaction. Sodium, being in group one, must lose one electron to have a complete outer electron shell and thus be stable.
What temperature is the reaction at equilibrium?
The temperature at which a reaction reaches equilibrium can vary depending on the specific reaction and its conditions. For some reactions, the temperature at equilibrium may be higher, while for others it may be lower. The equilibrium temperature is determined by the enthalpy change of the reaction and the equilibrium constant.
What does if it rain you wont get wet mean?
It means that under the given condition of rain, you will not get wet.
What redox conditions will produce a spontaneous reaction?
The sum of the voltages of the half-reactions is positive.
How does a voltiac cell work?
The voltaic cell work under the principle of redox reaction which involves the transfer of electrons from one electrode to another.
The cell potential of an electrochemical cell is positive. What does that tell you about the redox reaction?
A positive cell potential indicates that the redox reaction is spontaneous under standard conditions. This means that the reactants have a higher free energy than the products, leading to a favorable reaction that can occur without external energy input. Additionally, it suggests that the reduction half-reaction has a greater tendency to gain electrons compared to the oxidation half-reaction losing them.
Under what condition would pressure affect the reaction rate?
If the reaction occurs in the gas phase
What identifies a spontaneous redox reaction?
A spontaneous redox reaction is identified by a positive cell potential (E°) when measured under standard conditions, indicating that the reaction can occur without external energy input. This is often determined using the standard reduction potentials of the half-reactions involved; if the total cell potential is positive, the reaction is spontaneous. Additionally, spontaneity can be inferred from the Gibbs free energy change (ΔG), where a negative ΔG signifies that the reaction is thermodynamically favorable.
What can be said about a redox reaction that has a positive pontential?
A redox reaction with a positive standard electrode potential indicates that the reaction is spontaneous under standard conditions. This means that the tendency for the reduction half-reaction to occur is favored, making it more likely for the oxidizing agent to gain electrons. In practical terms, such reactions can drive processes like electrochemical cells, where energy is harnessed from the spontaneous electron transfer. Thus, a positive potential signifies a favorable thermodynamic outcome for 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.
What is the complete redox reaction for MnO4- and H2O2 under acid conditions?
2 H2O2 -- [MnO2] --> 2 H2O + O2 A catalyst does not take place in a chemical reaction, thus it cannot be placed at the reactant or product side of the reaction equation. In stead it is usually placed above the reaction arrows, sometimes between right brackets: -- [MnO2] -->
What following pieces of information is given in a half reaction?
A half-reaction provides information about either the oxidation or reduction process occurring in a redox reaction. It includes details about the species being oxidized or reduced, the electrons involved (with the number of electrons added or removed), and any relevant ions or molecules participating in the reaction. Additionally, it may specify the conditions under which the reaction occurs, such as the state of the reactants and products.
What is the overall voltage for the non spontaneous redox reaction Mg and Cu and their ions?
For the non-spontaneous redox reaction between magnesium (Mg) and copper ions (Cu²⁺), the overall cell voltage can be calculated using standard electrode potentials. The standard reduction potential for Cu²⁺/Cu is +0.34 V, while for Mg²⁺/Mg it is -2.37 V. The overall cell potential (E°) for the reaction is E° = E°(reduction) - E°(oxidation) = +0.34 V - (-2.37 V) = +2.71 V. However, since the reaction is non-spontaneous, the cell voltage would be negative under standard conditions, indicating that external energy is required to drive the reaction.
Is rust an example of a physical change or a chemical change?
It is an example of chemical change which cannot be reversed. In this change, Iron oxidizes under the presence of oxygen and moisture. The reaction is called a reduction-oxidation, or redox, reaction.
What is the overall voltage for the non-spontaneous redox reaction involving mg and cu and their ions?
In a redox reaction involving magnesium (Mg) and copper ions (Cu²⁺), magnesium is oxidized and copper is reduced. The standard reduction potential for Cu²⁺ to Cu is +0.34 V, while the standard reduction potential for Mg²⁺ to Mg is -2.37 V. The overall cell voltage (E°) for the reaction is calculated as the difference between these potentials: E° = E°(reduction) - E°(oxidation) = 0.34 V - (-2.37 V) = +2.71 V. Since this voltage is positive, the reaction is spontaneous under standard conditions, contrary to the premise of being non-spontaneous.
