chlorine was oxidized while oxygen was reduced to form hydrochloric acid.
In this reaction, FeCl2 is the oxidizing agent because it causes another species to be reduced (lose electrons), while SnCl2 is the reducing agent because it causes another species to be oxidized (gain electrons).
No, oxidized molecules have more energy than reduced molecules.
During battery discharge, the species that is oxidized is the anode.
During the electrochemical reaction, the anode is oxidized.
B. oxidized In this reaction, ethanol is oxidized to acetaldehyde, while manganese is reduced from a +7 oxidation state to a +2 oxidation state.
In the reaction MnO2 + 4HCl -> MnCl2 + Cl2 + 2H2O, manganese in MnO2 is getting oxidized from +4 to +2 (in MnCl2). Chloride ions in HCl are being reduced to chlorine gas (Cl2).
Oxidized.
The answer is not c.
yes
The way to tackle this to look at reactants and at the products, and this where oxidation numbers come in. Remembering that oxidation is loss of electrons and reduction is gain, (OILRIG is an acronym that is sometimes used). Mn metal is changed to Mn2+ so it is oxidised H in HCl has a +1 oxidation number and in H2 zero so it is reduced. Cl in HCL is at -1 and is -1 in MnCl2 so it is neither oxidised nor reduced.
In this reaction, FeCl2 is the oxidizing agent because it causes another species to be reduced (lose electrons), while SnCl2 is the reducing agent because it causes another species to be oxidized (gain electrons).
The iron is oxidized and the silver is reduced.
Water is oxidized in the process of photosynthesis.
No, oxidized molecules have more energy than reduced molecules.
During battery discharge, the species that is oxidized is the anode.
Photosynthesis is a redox reaction where water (H2O) is oxidized during the light reactions, leading to the release of oxygen as a byproduct. In the Calvin cycle, carbon dioxide (CO2) is reduced to form carbohydrates with the help of ATP and NADPH produced during the light reactions. Therefore, the correct options are c. oxidized...reduced.
During the electrochemical reaction, the anode is oxidized.