Answer:
Mass = 9.58 g    
Explanation:
Given data:
Mass of Fe₂O₃ formed = ?
Mass of Fe = 6.7 g
Solution:
Chemical equation:
4Fe + 3O₂        →    2Fe₂O₃
Number of moles of Fe:
Number of moles = mass/molar mass
Number of moles = 6.7 g/ 55.8 g/mol
Number of moles = 0.12 mol
now we will compare the moles of Fe and Fe₂O₃.
                          Fe         :          Fe₂O₃
                            4         :              2
                          0.12       :          2/4×0.12 = 0.06 mol
Mass of Fe₂O₃:
Mass = number of moles × molar mass
Mass = 0.06 mol  × 159.69 g/mol
Mass = 9.58 g    
 
        
             
        
        
        
Answer:
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Answer:

Explanation:
We can use the Ideal Gas Law to solve this problem
pV = nRT
Data:
p = 1.1 atm
n = 3.2 mol
R = 0.082 16 L·atm·K⁻¹mol⁻¹
T = 295 K
Calculation:

 
        
             
        
        
        
Answer:
a. 
b. 0.092 M
Explanation:
Hello!
In this case, since for this titration process we know the used volume of 0.75-M sodium hydroxide needed to neutralize 155 mL of the acid, we first need to write the undergoing chemical reaction between them:

This, since there is 1:2 mole ratio between the acid and the base, at the equivalent point we must respect:

That in terms of concentrations and volumes is:

Thus, the concentration of acid was:

Best regards!