Answer:
Electric current
Hydrogen and oxygen gas
Explanation:
Electrolysis is defined as a method of separation whereby an electric current is introduced into compounds to separate them . The electric current used here is a direct electric current (DC) and it makes the compound to be spit into its' component elements.
Now, in the case of water like it says in the question. Water is a mixture of hydrogen and oxygen gas. Thus, when electric current is passed through water which has an Electrolyte, it makes the water to decompose into its compound elements which are hydrogen and oxygen.
Answer is: between the carbon atom and the oxygen atom in a molecule of methanal there are two (2) <span>pairs of electrons.
Methanal or formaldehyde (H</span>₂C=O)<span> </span><span>is the simplest of the </span><span>aldehydes.
In methanal, bond between carbon and oxygen is double covalent bond (one sigma and one pi bond), which means there are four shared electrons or two pair of electrons.</span>
Examining the given reaction:
Li2O + H2O ........> 2LiOH
we find that, 1 mole of Li2O is required to react with one mole of H2O in order to produce two moles of LiOH.
Therefore, the ration between the required Li2O and H2O is 1:1
Based on this, 2.2 moles of H2O (water) are required to react with 2.2 moles of Li2O
Answer:
Exposure of silver chloride to sunlight for a long duration turns grey due to photolytic decomposition i.e decomposition in the presence of sunlight.
Explanation:
When silver chloride, AgCl is exposed to sunlight for a long time, it will undergo decomposition as the sunlight provides sufficient energy needed to decomposed the salt, AgCl to metallic silver and chlorine gas. This can be seen in the equation below:
2AgCl —> 2Ag + Cl2
Zinc would be considered the strongest reducing agent.
<h3>Reducing agent</h3>
A reducing agent is a chemical species that "donates" one electron to another chemical species in chemistry (called the oxidizing agent, oxidant, oxidizer, or electron acceptor). Earth metals, formic acid, oxalic acid, and sulfite compounds are a few examples of common reducing agents.
Reducers have excess electrons (i.e., they are already reduced) in their pre-reaction states, whereas oxidizers do not. Usually, a reducing agent is in one of the lowest oxidation states it can be in. The oxidation state of the oxidizer drops while the oxidizer's oxidation state, which measures the amount of electron loss, increases. The agent in a redox process whose oxidation state rises, which "loses/donates electrons," which "oxidizes," and which "reduces" is known as the reducer or reducing agent.
Learn more about reducing agent here:
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