Answer:
2.0 moles
Explanation:
Limiting reagent is the one which is present in small amount. The formation of the product is governed by the limiting reagent.
Given that:-
2.0 moles of A (with an excess of B) can make a maximum of 2.0 moles of C 3.0 moles of B (with an excess of A) can make a maximum of 4.0 moles of C
Thus,
Moles of C = moles of A = (4/3) moles of B
The balanced reaction may be:-
Given, moles of A = 2.0 moles
Moles of B = 3.0 moles
4 mole of A react with 3 moles of B
1 mole of A react with 3/4 moles of B
2 moles of A react with (3/4)*2 moles of B
Moles of B = 2.5 moles
Available moles of B = 3.0 moles
B is in excess. Thus, A is the limiting reagent.
4 mole of A produces 4 mole of C
Thus, C produced from 2 moles of A = 2.0 moles
Answer:it will shake up more
Explanation:the mass of it falling and means when open it will explode
Answer:
1. It is stoichiometric.
2. O2 is the limiting reactant.
3. 9.0 g of C2H6 remain unreacted.
4. 17.6 g of CO2.
5. 85.2%.
Explanation:
Hello there!
In this case, for the given chemical reaction:
We can see that:
1. It is stoichiometric and is balanced because the reactants yields the products according to the law of conservation of mass.
2. In this part, it is possible to calculate the moles of ethane by using its molar mass:
And the moles of oxygen by knowing that one mole is contained in 22.4 L at STP:
Thus, by calculating the moles of carbon dioxide product by each reactant, we can identify the limiting one:
Thus, since oxygen yields the fewest moles of CO2 product, we infer it is the limiting reactant.
3. In this part, we calculate the mass of C2H6 that actually react first:
Thus, the leftover of ethane (C2H6) as the excess reactant is:
4. Since 0.4 moles of carbon dioxide were produced, we use its molar mass to calculate the mass as its theoretical yield:
5. Finally, the percent yield is gotten by dividing the actual yield by the theoretical one:
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We call it a solid because it has the () and in s inside of it meaning solid