The reaction 2NO(g) + O2(g) → 2NO2(g)
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We have to solve this question using the stoichiometry of the reaction:
The equation of the reaction is;
According to the question;
Number of moles of CO2 released = 21.3 g/44 g/mol = 0.48 moles
From the stoichiometry of the reaction:
Since;
24 moles of CO2 released 15,026 KJ
0.48 moles of CO2 will release 0.48 * 15,026/24
= 301 KJ of heat.
<u>Answer:</u> The value of for the reaction will be -537 kJ
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of hydrogen gas = 0.647 g
Molar mass of hydrogen gas = 2 g/mol
Putting values in above equation, we get:
We are given:
Energy released for 0.324 moles of hydrogen reacted is 174 kJ
For the given chemical reaction:
By Stoichiometry of the reaction:
When 0.324 moles of hydrogen gas is reacted, the energy evolved is 174 kJ
So, when 1 mole of hydrogen gas will react, the energy evolved will be =
<u>Sign convention of heat:</u>
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
Hence, the value of for the reaction will be -537 kJ