How many grams of #H_2O# will be produced if 750 grams of #Fe# are produced in the equation #Fe_3O_4 + H_2 -> Fe + H_2O#?
Approx.....
I A stoichiometric equation is required.
And (ii) we calculate the corresponding amount of metal.
Thus, we accept the product.
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To solve this problem, we need to determine the stoichiometry of the reaction, which relates the amounts of reactants and products based on their molar ratios. From the balanced chemical equation:
Fe3O4 + 4H2 -> 3Fe + 4H2O
We see that for every 4 moles of H2 used, 4 moles of H2O are produced.
Next, we need to convert the given mass of Fe (750 grams) to moles. The molar mass of Fe is approximately 55.85 g/mol.
750 grams / 55.85 g/mol ≈ 13.43 moles of Fe
Since the ratio of H2 to H2O is 4:4 (or 1:1), the same number of moles of water will be produced.
Therefore, 13.43 moles of H2O will be produced.
Finally, we can convert moles of H2O to grams. The molar mass of water (H2O) is approximately 18.015 g/mol.
13.43 moles × 18.015 g/mol ≈ 241.77 grams of H2O.
So, approximately 241.77 grams of H2O will be produced.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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