<span>when density in g/ml
9.86ml CH3COOH (X g/1ml) = g
1.049g/ml
9.86ml (1.049g/1ml) = 10.343 g
hope it helps
</span>
<span>C. A completely new substance is formed.</span>
The balanced skeleton reactions are given below
2CrO₄²⁻(aq) + 3Cu(s) +8
(l) → 2Cr(OH)₃(s) + 3Cu(OH)₂(s) + 6
(aq)
The oxidising agent and reducing agents are Cr and Cu .
There are following steps involve in balance redox reaction in basic medium .
- First divide the reaction into two half reactions which give oxidation and reduction half reaction.
- Then balance the elements other than oxygen and hydrogen atom.
- Balance the oxygen atom by adding where number of oxygen is less .
- Balance the hydrogen atom by adding
on another side of where water molecule added. - Add ions to both sides to neutralize ion.
- Combine and ion to make .
- Balance the charge by adding
.
The species which reduces the other species in the redox reaction is called oxidizing agent . Similarly , the species which oxidize the other species in the redox reaction is called reducing agent .
To learn more about reducing agents please click here ,
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The answer would be B. Liquid
Explanation:
An oxidizing agent is a reactant that removes electrons from other reactants during a redox reaction. The oxidizing agent typically takes these electrons for itself, thus gaining electrons and being reduced. An oxidizing agent is thus an electron acceptor.
Examples of Oxidizing Agents include the following; Hydrogen peroxide, ozone, oxygen.
A half-equation shows you what happens at one of the electrodes during electrolysis . Electrons are shown as e -. A half-equation is balanced by adding, or taking away, a number of electrons equal to the total number of charges on the ions in the equation.
The balanced half reaction equation for H2O2 as an oxidizing agent is given as;
H2O2 + 2e^- + 2H^+ ==> 2H2O
