The rock in a particular iron ore deposit contains 84 % Fe2O3 by mass.
How many kilograms of the rock must be processed to obtain 1100 kg of iron?
Fe2O3 ==> 2Fe so you see there are 2 mols Fe in 2 mol Fe2O3.
To get 1100 kg Fe will require
1100 kg Fe x (1 mol Fe2O3/2 mols Fe) = about 550 kg Fe2O3. That is only 84% Fe2O3 in the ore itself; therefore, 550/0.84 = ? kg of the ore.
Why did the rock go to therapy? Because it had an iron deficiency! But don't worry, I've got the answer for you.
To determine how many kilograms of the rock must be processed to obtain 1100 kg of iron, we need to calculate the mass of Fe2O3 in the rock.
Given that the rock contains 84% Fe2O3 by mass, we can set up the following equation:
Mass of Fe2O3 = (84/100) * Mass of the rock
Now, since the total mass of the rock contains the mass of Fe2O3 and other components, we can write:
Mass of the rock = Mass of Fe2O3 + Mass of other components
We know that the mass of Fe2O3 is equal to 1100 kg (since that's the desired amount of iron), so we can rearrange the equation to solve for the mass of the rock:
Mass of the rock = Mass of Fe2O3 + Mass of other components
Mass of the rock = 1100 kg + Mass of other components
However, we don't know the exact mass of the other components, so we'll have to leave it as a variable.
So, to answer your question, we don't have enough information to determine the exact mass of the rock that needs to be processed. We need to know the mass of the other components in the rock. But hey, at least we had a good laugh along the way!
To determine the amount of iron in the rock, we need to consider the mass percentage of Fe2O3.
Given that the rock contains 84% Fe2O3 by mass, we know that the remaining 16% is comprised of other substances.
To calculate the mass of Fe2O3 in the rock, we can use the following formula:
Mass of Fe2O3 = (Mass percentage of Fe2O3 / 100) x Mass of the rock
Let's assume the mass of the rock as 'x' kg. Therefore, the mass of Fe2O3 in the rock is:
Mass of Fe2O3 = (84/100) x x = 0.84x kg
Now, we need to determine the mass of iron (Fe) in the Fe2O3. In Fe2O3, there is a 2:3 ratio of Fe to Fe2O3. So, the mass of iron in the rock is:
Mass of iron = (mass of Fe2O3 / molecular weight of Fe2O3) x molecular weight of Fe
= (0.84x / (2 x atomic weight of Fe + 3 x atomic weight of O)) x atomic weight of Fe
Given that the atomic weight of Fe is approximately 55.85 g/mol, we can use this value to calculate the mass of iron in the rock.
Now, we need to determine the mass of iron (Fe) that we want to obtain, which is 1100 kg.
Setting up an equation:
Mass of iron = Mass of Fe2O3 - Mass of rock
Substituting the values we calculated previously:
1100 kg = (0.84x / (2 x atomic weight of Fe + 3 x atomic weight of O)) x atomic weight of Fe - x kg
Now, we can solve this equation to find the value of x, which represents the mass of the rock in kilograms.
To answer this question, we need to calculate the mass of iron in the rock containing 84% Fe2O3 and then determine the amount of rock needed to obtain 1100 kg of iron.
Step 1: Calculate the mass of iron in the rock.
Since the rock contains 84% Fe2O3, we can assume that the remaining mass (100% - 84% = 16%) is other elements/non-iron components. So, the iron content in the rock is 84% of the total mass.
Iron content = 84% of the total mass
= 84/100 * mass of rock
Step 2: Determine the amount of rock needed to obtain 1100 kg of iron.
Since the mass of iron obtained from the rock will be 1100 kg, we can set up the following equation:
Iron content = 1100 kg
So, we can solve for the mass of the rock using the iron content calculated in step 1:
84/100 * mass of rock = 1100 kg
To find the mass of rock, we can rearrange the equation:
mass of rock = 1100 kg * 100/84
Now, let's calculate the mass of rock:
mass of rock = 1100 kg * 100/84
= 1309.52 kg
Therefore, approximately 1309.52 kg of the rock must be processed to obtain 1100 kg of iron.