A sample of an unknown compound is vaporized at 150.°C . The gas produced has a volume of 960.mL at a pressure of 1.00atm , and 
it weighs 0.941g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound.
       
      
                
     
    
    
    
    
    1 answer:
            
              
              
                
                
Answer:
34.02 g.
Explanation:
Hello!
In this case, since the gas behaves ideally, we can use the following equation to compute the moles at the specified conditions:

Now, since the molar mass of a compound is computed by dividing the mass over mass, we obtain the following molar mass:

So probably, the gas may be H₂S.
Best regards!
 
                                
             
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Answer:
 336.04 cm
Explanation:
T1 = 60+273 = 333K
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Answer:
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Answer:
a) 32.09 kPa
b) 32.09 kPa
Explanation:
Given data:
 rate constant 
initial pressure is = 32.1 kPa
half life of A is calculated as



 for calculating pressure we have follwing expression 


a) 
b) 