Calculate the volume (in mL) of 9.0M H2SO4 that you would need to convert 0.070 moles of KAl(OH)4 to K2SO4 and Al2(SO4)3 according to the following equation:
2 KAl(OH)4 + 4 H2SO4 --> K2SO4 + Al2(SO4)3 + 8 H2O
Well, if I could calculate that for you, I would be one very talented Clown Bot! But lucky for you, I happen to know a thing or two about chemistry.
First, let's find out the number of moles of H2SO4 needed to convert 0.070 moles of KAl(OH)4. According to the balanced equation, it tells us that it takes 4 moles of H2SO4 to react with 2 moles of KAl(OH)4.
So, if we have 0.070 moles of KAl(OH)4, we will need half the amount of H2SO4. Therefore, we need 0.035 moles of H2SO4.
Now, let's convert the moles of H2SO4 into milliliters (ml). Since we have a 9.0M H2SO4 solution, this means we have 9.0 moles of H2SO4 in 1 liter (1000 ml) of solution.
So, to find the volume of 0.035 moles of H2SO4, we can use the following equation:
Volume (ml) = (moles of H2SO4 / molarity of H2SO4) * 1000
Plugging in the values, we get:
Volume (ml) = (0.035 moles / 9.0 M) * 1000
= 3.89 ml
So, approximately 3.89 milliliters of 9.0M H2SO4 would be needed to convert 0.070 moles of KAl(OH)4.
To calculate the volume of 9.0M H2SO4 required to convert 0.070 moles of KAl(OH)4, we need to use the equation provided as a stoichiometry conversion factor.
The balanced equation is:
2 KAl(OH)4 + 4 H2SO4 → K2SO4 + Al2(SO4)3 + 8 H2O
From the equation, we know that 2 moles of KAl(OH)4 react with 4 moles of H2SO4.
Now we can set up the conversion:
0.070 moles KAl(OH)4 x (4 moles H2SO4 / 2 moles KAl(OH)4) x (1 liter / 9.0 moles H2SO4) x (1000 mL / 1 liter)
Let's calculate it step by step:
Step 1:
0.070 moles KAl(OH)4 x (4 moles H2SO4 / 2 moles KAl(OH)4) = 0.140 moles H2SO4
Step 2:
0.140 moles H2SO4 x (1 liter / 9.0 moles H2SO4) = 0.0156 liters
Step 3:
0.0156 liters x (1000 mL / 1 liter) ≈ 15.6 mL
Therefore, you would need approximately 15.6 mL of 9.0M H2SO4 to convert 0.070 moles of KAl(OH)4 according to the given equation.
To calculate the volume of 9.0M H2SO4 needed, we can use the given balanced chemical equation and the stoichiometry of the reaction.
Step 1: Convert moles of KAl(OH)4 to moles of H2SO4
From the balanced equation, we can see that 2 moles of KAl(OH)4 react with 4 moles of H2SO4. Therefore, the mole ratio between KAl(OH)4 and H2SO4 is 2:4 or 1:2.
Given that we have 0.070 moles of KAl(OH)4, we can convert that to moles of H2SO4 using the mole ratio:
0.070 moles KAl(OH)4 * (2 moles H2SO4 / 1 mole KAl(OH)4) = 0.14 moles H2SO4
Step 2: Convert moles of H2SO4 to volume of H2SO4
We are given the concentration of H2SO4 as 9.0M (moles per liter or mol/L). The concentration tells us that in 1 liter (1000 mL) of H2SO4 solution, there are 9 moles of H2SO4.
To find the volume of H2SO4 required for 0.14 moles, we can use the following calculation:
Volume of H2SO4 (in mL) = (0.14 moles H2SO4) * (1000 mL / 9 moles)
Volume of H2SO4 = (0.14 * 1000) / 9 ≈ 15.56 mL (rounded to two decimal places)
Therefore, you would need approximately 15.56 mL of 9.0M H2SO4 to convert 0.070 moles of KAl(OH)4 to K2SO4 and Al2(SO4)3.