Answer:
B) 16 g
Explanation:
First we <u>convert 4 moles of O₂ into moles of H₂</u>, using the <em>stoichiometric coefficients of the balanced reaction</em>:
- 4 mol O₂ *  = 8 mol H₂ = 8 mol H₂
Finally we <u>convert 8 moles of H₂ into grams</u>, using <em>its molar mass</em>:
- 8 mol H₂ * 2 g/mol = 16 g
Thus, the correct answer is option B).
 
        
             
        
        
        
Answer:
Explanation:
From the given information:
TO start with the molarity of the solution:

= 0.601 mol/kg
= 0.601 m
At the freezing point, the depression of the solution is 

Using the depression in freezing point, the molar depression constant of the solvent 


The freezing point of the solution 

The molality of the solution is:

Molar depression constant of solvent X, 
Hence, using the elevation in boiling point;
 the Vant'Hoff factor 


 
        
             
        
        
        
Answer:
Explanation:
Given parameters : 
Volume of solution  = 100mL 
Absorbance of solution  = 0.30
Unknown: 
Concentration of CuSO₄ in the solution = ? 
Solution: 
There is relationship between the absorbance and concentration of a solution. They are directly proportional to one another. 
A graph of absorbance against concentration gives a value of 0.15M at an absorbance of 0.30. 
The concentration is 0.15M
Also, we can use:  Beer-Lambert's law; 
                     A  = ε mC l
where εm is the molar extinction coefficient
              C is the concentration 
              l is the path length
Since the εm is not given and assuming path length is 1; 
          Then we solve for the concentration. 
 
        
             
        
        
        
Answer:
CaCO3 -> CaO + CO2
Explanation:
Woahhhh, did you balance it yourself just then?
 
        
             
        
        
        
<span>Although two centuries old, Dalton's atomic theory remains valid in modern chemical thought. 1) All matter is made of atoms. Atoms are indivisible and indestructible. 3) Compounds are formed by a combination of two or more different kinds of atoms.</span>