Please help! I don't understand these questions at all. :(
Fe2O3(s) + 2Al(s) -> Al2O3(s) + 2Fe(l)
If 0.50 mol of Fe is produced in 10 secs, what is the rate of consumption of Fe2O3 in mol/s?
A. 5.0 x 10^-2 mol/s
B. 2.5 x 10^-2 mol/s
C. 1.0 x 10^-1mol/s
D. 5.0 mol/s
Thank you!
These problems are worked the same as a stoichiometry problem. That is,
0.5 mol Fe/10s = 0.05 mol/s, then convert to Fe2O3 by
0.05 mols/x x (1 mol Fe2O3)/2 mols Fe) = 0.025 mol Fe2O3/s.
To find the rate of consumption of Fe2O3, we need to use the coefficients from the balanced chemical equation to calculate the stoichiometry.
From the equation, we can see that 1 mole of Fe2O3 reacts to produce 2 moles of Fe.
Given that 0.50 mol of Fe is produced in 10 seconds, we can find the amount of Fe2O3 consumed using the stoichiometry.
Using the ratio of 1 mole Fe2O3 to 2 moles Fe, we can set up a proportion to find the amount of Fe2O3 consumed:
(0.50 mol Fe / 2 mol Fe) = (x mol Fe2O3 / 1 mol Fe2O3)
Cross-multiplying, we get:
0.50 mol Fe2O3 = 2 * x mol Fe
0.50 mol Fe2O3 = 2x
Dividing both sides by 2, we get:
0.25 mol Fe2O3 = x
Therefore, the rate of consumption of Fe2O3 is 0.25 mol/s.
So the correct answer is C. 1.0 x 10^-1 mol/s.
To find the rate of consumption of Fe2O3 in mol/s, we need to use the stoichiometric coefficients from the balanced chemical equation.
First, let's identify the stoichiometric coefficients for Fe2O3 and Fe in the balanced chemical equation:
Fe2O3(s) + 2Al(s) -> Al2O3(s) + 2Fe(l)
From the equation, we can see that for every 1 mole of Fe2O3 consumed, 2 moles of Fe are produced.
Given that 0.50 mol of Fe is produced in 10 s, we can use this information to find the rate of Fe2O3 consumption.
Step 1: Calculate the moles of Fe2O3 consumed.
Since the stoichiometric ratio is 1:1 between Fe2O3 and Fe, the same number of moles of Fe2O3 must be consumed as the number of moles of Fe produced. Therefore, if 0.50 mol of Fe is produced, 0.50 mol of Fe2O3 must be consumed.
Step 2: Calculate the rate of Fe2O3 consumption.
The rate of Fe2O3 consumption is determined by dividing the amount of Fe2O3 consumed by the time taken. In this case, the time taken is 10 s.
Rate of Fe2O3 consumption = Amount of Fe2O3 consumed / Time taken
Rate of Fe2O3 consumption = 0.50 mol / 10 s
Rate of Fe2O3 consumption = 0.05 mol/s
Therefore, the rate of consumption of Fe2O3 is 0.05 mol/s.
Now, let's match this value to the given options:
A. 5.0 x 10^-2 mol/s
B. 2.5 x 10^-2 mol/s
C. 1.0 x 10^-1 mol/s
D. 5.0 mol/s
The rate calculated is 0.05 mol/s, which is equal to 5.0 x 10^-2 mol/s. So, the correct answer is A. 5.0 x 10^-2 mol/s.