how many grams of lithium sulfate will be formed when 25 grams of sulfuric acid react with an excess of lithium hydroxide in the following reaction
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To determine the number of grams of lithium sulfate formed, we need to:
Step 1: Write the balanced chemical equation for the reaction between sulfuric acid (H2SO4) and lithium hydroxide (LiOH):
H2SO4 + 2LiOH -> Li2SO4 + 2H2O
Step 2: Calculate the molar mass of sulfuric acid (H2SO4) and lithium sulfate (Li2SO4):
Molar mass of H2SO4 = 1 * 2 (hydrogen) + 32.1 (sulfur) + 16 * 4 (oxygen) = 98.1 g/mol
Molar mass of Li2SO4 = 6.9 * 2 (lithium) + 32.1 (sulfur) + 16 * 4 (oxygen) = 109.9 g/mol
Step 3: Identify the molar ratio between sulfuric acid (H2SO4) and lithium sulfate (Li2SO4) from the balanced chemical equation:
From the balanced chemical equation, we can see that 1 mole of H2SO4 corresponds to 1 mole of Li2SO4.
Step 4: Convert the given mass of sulfuric acid (H2SO4) into moles:
Moles of H2SO4 = given mass of H2SO4 / molar mass of H2SO4
= 25 g / 98.1 g/mol
≈ 0.255 moles
Step 5: Determine the number of moles of lithium sulfate (Li2SO4) formed using the molar ratio:
Moles of Li2SO4 = Moles of H2SO4
Therefore, moles of Li2SO4 ≈ 0.255 moles.
Step 6: Convert moles of lithium sulfate (Li2SO4) into grams:
Mass of Li2SO4 = moles of Li2SO4 * molar mass of Li2SO4
= 0.255 moles * 109.9 g/mol
≈ 27.9 grams
So, approximately 27.9 grams of lithium sulfate will be formed when 25 grams of sulfuric acid react with an excess of lithium hydroxide.
To determine the number of grams of lithium sulfate formed in the reaction, we need to balance the chemical equation first.
The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and lithium hydroxide (LiOH) is:
H2SO4 + 2LiOH -> Li2SO4 + 2H2O
From the balanced equation, we can see that 1 mole of sulfuric acid (H2SO4) reacts with 2 moles of lithium hydroxide (LiOH) to produce 1 mole of lithium sulfate (Li2SO4).
Step 1: Convert the given mass of sulfuric acid (H2SO4) to moles.
To do this, we need to know the molar mass of sulfuric acid, which is 98.08 grams/mol.
moles of H2SO4 = mass of H2SO4 / molar mass of H2SO4
moles of H2SO4 = 25 grams / 98.08 grams/mol ≈ 0.254 moles
Step 2: Determine the moles of lithium sulfate formed.
From the balanced equation, we know that the moles of sulfuric acid (H2SO4) reacting are equal to the moles of lithium sulfate (Li2SO4) formed. In this case, it is 0.254 moles.
Step 3: Convert the moles of lithium sulfate to grams.
To do this, we need to know the molar mass of lithium sulfate, which is 109.94 grams/mol.
mass of Li2SO4 = moles of Li2SO4 x molar mass of Li2SO4
mass of Li2SO4 = 0.254 moles x 109.94 grams/mol ≈ 27.95 grams
Therefore, approximately 27.95 grams of lithium sulfate will be formed when 25 grams of sulfuric acid reacts with an excess of lithium hydroxide in the given reaction.