The reaction will produce 12.1 g Ag₂S.
<em>Balanced equation</em> = 2Ag + S ⟶ Ag₂S
<em>Mass of Ag₂S</em> = 10.5 g Ag × (1 mol Ag/107.87 g Ag) × (1 mol Ag₂S/2 mol Ag)
× (247.80 g Ag₂S/1 mol Ag₂S) = 12.1 g Ag₂S
 
        
             
        
        
        
Answer:
The answer is
<h2>2.00 %</h2>
Explanation:
The percentage error of a certain measurement can be found by using the formula

From the question
actual measurement = 46.37 g
error = 47.25 - 46.37 = 0.88 
The percentage error of the measurement is

We have the final answer as
<h3>2.00 %</h3>
Hope this helps you
 
        
             
        
        
        
Both figures are mixtures,
Figure II is a heterogenous mixture
Figure I is a homogenous mixture
 
        
             
        
        
        
Answer : The partial pressure of the  in the tank in psia is, 32.6 psia.
 in the tank in psia is, 32.6 psia.
Explanation :
As we are given 75 %  and 25 %
 and 25 %  in terms of volume.
 in terms of volume.
First we have to calculate the moles of  and
 and  .
.


Now we have to calculate the mole fraction of  .
.


Now we have to calculate the partial pressure of the  gas.
 gas.


conversion used : (1 Kpa = 0.145 psia)
Therefore, the partial pressure of the  in the tank in psia is, 32.6 psia.
 in the tank in psia is, 32.6 psia.
 
        
             
        
        
        
Answer:
Bi (Bismuth)
Ag (Silver)
Li (Lithium)
Explanation:
Xe (Xenon) and I (Iodine) are non-metals. They cannot from a metallic bond because metallic bonds are bonds between metals only.