<h3>Answer:</h3>
                  162.43 g of FeCl₂
<h3>
Explanation:</h3>
Step 1: Calculate mass of Fe;
As,
                                    Density  =  Mass ÷ Volume
Or,
                                    Mass  =  Density × Volume
Where Volume is the volume of water displaced  =  10.4 mL
Putting values,
                                    Mass  =  7.86 g.mL⁻¹ × 10.4 mL
                                    Mass  =  81.744 g of Fe
Step 2: Calculate amount of FeCl₂;
The balance chemical equation is as follow,
                                 Fe  +  2 HCl   →    FeCl₂  +  H₂ ↑
According to this equation,
        55.85 g (1 mol) Fe produced  =  110.98 g (1 mol) of FeCl₂
So,
                81.744 g Fe will produce  =  X g of FeCl₂
Solving for X,
                      X  =  (81.744 g × 110.98 g) ÷ 55.85 g
                      X  =  162.43 g of FeCl₂
 
        
        
        
The region is located on an active oceanic plate
        
             
        
        
        
The balanced equation given is:
4NH3 + 3O2 .....> 2N2 + 6H2O
From this equation, we can note that 4 moles of NH3 are required to produce 2 moles of N2.
Therefore, the mole ratio of NH3 to N2 is 4:2 which can be simplified into 2:1
        
                    
             
        
        
        
Bcz you’re able to wear something fresh, get a tan if you’d want, play volleyball or go out to swim in the cold ocean that feels so good when it’s hot !
        
                    
             
        
        
        
Answer : The correct option is, 
Explanation :
- Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. That means, the loss of electrons takes place.
Or we can say that, oxidation reaction occurs when a reactant losses electrons in the reaction.
- Reduction reaction : It is defined as the reaction in which a substance gains electrons. That means, the gain of electrons takes place.
Or we can say that, reduction reaction occurs when a reactant gains electrons in the reaction.
According to the electrochemical series,  most likely to be reduced because
 most likely to be reduced because 
Hence, the ion most likely to be reduced is  .
.