A compound with the empirical formula NPCl2 was found in a subsequent experiment to have a molar mass of 347.64 g/mol. What is t
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<u>Answer:</u> The enthalpy of the reaction is coming out to be -902 kJ.
<u>Explanation:</u>
Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as
The equation used to calculate enthalpy change is of a reaction is:
For the given chemical reaction:
The equation for the enthalpy change of the above reaction is:
We are given:
Putting values in above equation, we get:
Hence, the enthalpy of the reaction is coming out to be -902 kJ.
<u>Answer:</u> The amount of carbon dioxide gas produced in the reaction is 83.6 grams
<u>Explanation:</u>
As, some amount of oxygen gas is left after the reaction is completed. So, it is present in excess and is considered as an excess reagent.
Thus, carbon is considered as a limiting reagent because it limits the formation of product.
To calculate the number of moles, we use the equation:
.....(1)
Given mass of carbon = 22.8 g
Molar mass of carbon = 12 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of carbon and oxygen gas follows:
By Stoichiometry of the reaction:
1 mole of carbon produces 1 mole of carbon dioxide gas
So, 1.9 moles of carbon will produce = of carbon dioxide gas
Now, calculating the mass of carbon dioxide from equation 1, we get:
Molar mass of carbon dioxide = 44 g/mol
Moles of carbon dioxide = 1.9 moles
Putting values in equation 1, we get:
Hence, the amount of carbon dioxide gas produced in the reaction is 83.6 grams