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A student wants to prove the concept of limiting reactants to his lab group during class. If the student adds 56 g or Fe to 71 g of Cl2, what will the likely result of the reaction be in regards to limiting/excess reactants?

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The result of the reaction will be such that Cl2 is limiting in its availability

Limiting reactants

From the equation of the reaction:

2Fe + 3Cl2 ---> 2FeCl3

Mole ratio of Fe and Cl2 = 2:3

Mole of 56 g of Fe = 56/56 = 1

Mole of 71 g of Cl2 = 71/71 = 1

Whereas, 1 mole of Fe requires 1.5 moles of Cl2. Thus, Cl2 is limiting in availability.

More on limiting reactants can be found here: https://brainly.com/question/14225536

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