What mass of sulfuric acid, H2SO4, is required to react with 3.27 g of potassium hydroxide, KOH? The products of this reaction are potassium sulfate
and water.
Have both the unbalanced and balanced chemical equations.
Explain how to find the molar mass of the compounds.
Explain how the balanced chemical equation is used to find the ratio of
Explain how many significant figures your answer needs to have.
The numerical answer
unbalanced: ... KOH + H2SO4 --> K2SO4 + H2O
balanced:.......2KOH + H2SO4 --> K2SO4 + 2H2O
Find molar mass by adding the atomic masses of the elements: for example, for H2SO4 that is 2*1 + 1*32 + 4*16 = 96
mols KOH = grams/molar mass KOH = 3.27/56 = 0.583
Convert mols KOH to mols H2SO4 using the coefficients in the balanced equation. 0.583 mols KOH x (1 mol H2SO4/2 mols kOH) = 0.583/2 = ?
Now convert mols H2SO4 to grams H2SO4. g H2SO4 = mols H2SO4 x molar mass H2SO4 = ? g
You may have two significant figures in the final answer using the numbers I've used. If you use 3 figures for the molar mass you may have 3 significant figures in the answer since the initial value is 3.27 g.
Unbalanced Chemical Equation:
H2SO4 + KOH → K2SO4 + H2O
Balanced Chemical Equation:
2H2SO4 + 2KOH → K2SO4 + 2H2O
To find the molar mass of the compounds, we need to add up the atomic masses of all the atoms in each compound.
The molar mass of H2SO4 can be calculated by adding up the atomic masses of each element:
Molar mass of H2SO4 = (2 * atomic mass of H) + atomic mass of S + (4 * atomic mass of O)
Similarly, the molar mass of KOH can be calculated by adding up the atomic masses of each element:
Molar mass of KOH = atomic mass of K + atomic mass of O + atomic mass of H
To find the ratio of the reactants and products, we use the coefficients in the balanced chemical equation.
In the balanced equation, we see that 2 moles of H2SO4 react with 2 moles of KOH to produce 1 mole of K2SO4 and 2 moles of H2O. This means that the ratio of H2SO4 to KOH is 2:2 or 1:1.
To calculate the mass of H2SO4 required to react with 3.27 g of KOH, we first need to determine the number of moles of KOH:
Number of moles of KOH = mass of KOH / molar mass of KOH
Next, we use the stoichiometry of the balanced equation to find the number of moles of H2SO4:
Number of moles of H2SO4 = Number of moles of KOH * (2 moles of H2SO4 / 2 moles of KOH)
Finally, we calculate the mass of H2SO4 by multiplying the number of moles of H2SO4 by its molar mass:
Mass of H2SO4 = Number of moles of H2SO4 * molar mass of H2SO4
To follow significant figures, we need to determine the limiting reagent. In this case, we compare the number of moles of H2SO4 to the number of moles of KOH. The reactant that produces fewer moles of the product will be the limiting reagent.
Finally, the numerical answer should be rounded to the smallest number of significant figures obtained from the given values used in the calculations.
The unbalanced chemical equation for the reaction between sulfuric acid (H2SO4) and potassium hydroxide (KOH) is:
H2SO4 + KOH -> K2SO4 + H2O
To find the molar masses of the compounds, you can use the periodic table. The molar mass of an element is the atomic mass of that element, which is usually listed on the periodic table. So, for sulfuric acid (H2SO4), you would find the molar mass by adding up the atomic masses of each element in the compound: 2(1.01 g/mol for hydrogen) + 32.07 g/mol for sulfur + 4(16.00 g/mol for oxygen). This gives you a molar mass of 98.09 g/mol for sulfuric acid. Similarly, for potassium hydroxide (KOH), you would calculate the molar mass as 39.10 g/mol for potassium + 16.00 g/mol for oxygen + 1.01 g/mol for hydrogen, giving you a molar mass of 56.11 g/mol for potassium hydroxide.
To balance the chemical equation, you need to make sure that the number of atoms of each element is the same on both sides of the equation. In this case, we have 2 hydrogen atoms on the left side and 2 hydrogen atoms on the right side, so that is already balanced. We have 1 sulfur atom on the left side and 1 sulfur atom on the right side, so that is also balanced. However, we have 4 oxygen atoms on the left side (2 from sulfuric acid and 2 from potassium hydroxide) and only 1 oxygen atom on the right side (from water). To balance the oxygen atoms, we need to put a coefficient of 4 in front of the water molecule on the right side:
H2SO4 + KOH -> K2SO4 + 4 H2O
Using the balanced equation, we can determine the stoichiometric ratio between sulfuric acid (H2SO4) and potassium hydroxide (KOH). From the equation, we can see that the ratio is 1:1. This means that for every mole of sulfuric acid, we need 1 mole of potassium hydroxide.
To find the mass of sulfuric acid required to react with 3.27 g of potassium hydroxide, we need to use the molar mass and the stoichiometric ratio.
First, calculate the number of moles of potassium hydroxide using its molar mass:
Moles of KOH = mass (g) / molar mass (g/mol)
Moles of KOH = 3.27 g / 56.11 g/mol ≈ 0.058 moles
Since the stoichiometric ratio is 1:1, the number of moles of sulfuric acid required will be the same as the moles of potassium hydroxide:
Moles of H2SO4 = 0.058 moles
Now, calculate the mass of sulfuric acid using its molar mass:
Mass of H2SO4 = moles of H2SO4 * molar mass of H2SO4
Mass of H2SO4 = 0.058 moles * 98.09 g/mol ≈ 5.68 g
Therefore, the mass of sulfuric acid required to react with 3.27 g of potassium hydroxide is approximately 5.68 g.
In terms of significant figures, the answer should have the same number of significant figures as the given value with the lowest number of significant figures. In this case, the given value is 3.27 g, which has three significant figures. Therefore, the final answer should also have three significant figures: 5.68 g.
FYI, your chemistry teacher knows that you are plagiarizing from here.
-From said chemistry teacher