<span>c. q = 0.75 g x 0.897 j/g•°c x 22°c</span>
This equation C5H + O2 ---> CO2 + H2O has a mistake.
C5H is wrong. You missed the subscript of H.
I will do it for you assuming some subscript to show you the procedure, but you have to use the right equation to get the right balanced equation.
Assuming the tha combustion equation is C5H12 + O2 ---> CO2 + H2O
First you need to balance C, so you put a 5 before CO2 and get
C5H12 + O2 ---> 5CO2 + H2O
Now you count the hydrogens: 12 on the left and 2 on the right. So put a 6 before H2O and get:
C5H12 + O2 ---> 5CO2 + 6H2O
Now count the oxygens: 2 on the left and 16 on the right, so put an 8 on before O2:
=> C5H12 + 8O2 ---> 5CO2 + 6H2O.
You can verify that the equation is balanced
To solve this we need to have knowledge of differential rate law which relate the rate to the concentration and time. Therefore, the rate of overall reaction is 1x10⁻²M/s.
<h3>
What is differential rate law? </h3>
A differential rate law represents the rate of a reaction . According to this rate is directly proportional to changes in the concentration of reactants and inversely proportional to specific interval of time. There is another expression of rate law which is integrated rate law which is just opposite of differential rate law.
The given equation is
2NO + O 2NO
(1/2) Rate of disappearance of NO= rate of disappearance of C= (1/2)rate of appearance of NO= rate of overall reaction.
(1/2)rate of appearance of NO= rate of overall reaction.
rate of appearance of NO=2x10⁻²M/s.
Substituting the values in above equation
(1/2)×2x10⁻²M/s = rate of overall reaction.
rate of overall reaction= 1x10⁻²M/s
Therefore, the rate of overall reaction is 1x10⁻²M/s.
To know more about differential rate law, here:
brainly.com/question/14821651
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