Answer :
Final answer:
There will be some excess mass of Nitrogen gas left un-reacted.
Explanation:
In this question, we are given that 84g of Nitrogen gas reacts with 128g of Oxygen gas to produce N204 gas. To determine the amount of excess mass left un-reacted, we need to first identify the limiting reactant.
To do this, we can calculate the moles of each reactant using their molar masses. The molar mass of Nitrogen gas (N2) is 28 g/mol, and the molar mass of Oxygen gas (O2) is 32 g/mol.
Using the given masses, we can calculate the moles of Nitrogen gas and Oxygen gas:
- Moles of Nitrogen gas = 84g / 28 g/mol = 3 moles
- Moles of Oxygen gas = 128g / 32 g/mol = 4 moles
From the balanced chemical equation, we can see that the ratio of moles of Nitrogen gas to Oxygen gas is 1:2. Therefore, Nitrogen gas is the limiting reactant because it is present in a lesser amount.
Now, let's calculate the theoretical mass of N204 gas that can be formed using the moles of Nitrogen gas:
- Moles of N204 gas = 3 moles of Nitrogen gas x (1 mole of N204 gas / 2 moles of Nitrogen gas) = 1.5 moles
The molar mass of N204 gas is 92 g/mol. Therefore, the theoretical mass of N204 gas that can be formed is:
- Theoretical mass of N204 gas = 1.5 moles x 92 g/mol = 138 g
Since the actual mass of N204 gas formed is not given, we cannot determine the exact amount of excess mass left un-reacted. However, we can conclude that there will be some excess mass of Nitrogen gas left un-reacted because it is the limiting reactant.
Learn more about excess mass in chemical reactions here:
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