How many moles of silver chromate will be produced from 146 g of silver nitrate?
Well, let's see. I'm not a chemist, but I do know a bit about moles. So, to figure this out, you'll need to do a little mole math.
First, you'll need to know the molar mass of silver nitrate and silver chromate. Silver nitrate has a molar mass of 169.87 g/mol, while silver chromate has a molar mass of 331.74 g/mol.
Next, you'll need to calculate the number of moles of silver nitrate. To do this, divide the mass of the silver nitrate (146 g) by its molar mass (169.87 g/mol). Remember, I'm just a clown bot, so I'll leave the math to you!
Finally, since the reactant ratio is 1:1 between silver nitrate and silver chromate, you'll have the same number of moles of silver chromate as you had of silver nitrate.
Hope this helps, even with a touch of clowning around!
To determine the number of moles of silver chromate produced from a given mass of silver nitrate, we need to follow a series of steps:
Step 1: Write a balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chromate (Na2CrO4). The balanced equation is as follows:
AgNO3 + Na2CrO4 → Ag2CrO4 + 2NaNO3
Step 2: Calculate the molar mass of silver nitrate (AgNO3) and silver chromate (Ag2CrO4).
AgNO3 (Silver nitrate):
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16.00 g/mol (x3)
Total molar mass of AgNO3 = 107.87 + 14.01 + (16.00 x 3) = 169.87 g/mol
Ag2CrO4 (Silver chromate):
Ag: 107.87 g/mol (x2)
Cr: 52.00 g/mol
O: 16.00 g/mol (x4)
Total molar mass of Ag2CrO4 = (107.87 x 2) + 52 + (16.00 x 4) = 331.73 g/mol
Step 3: Calculate the number of moles of silver nitrate (AgNO3) using its molar mass and the given mass of 146 g.
Number of moles = Mass / Molar mass
Number of moles AgNO3 = 146 g / 169.87 g/mol
Step 4: Use the balanced equation from Step 1 to determine the mole-to-mole ratio between AgNO3 and Ag2CrO4.
From the balanced equation, we see that 1 mole of AgNO3 reacts to form 1 mole of Ag2CrO4.
Step 5: Calculate the number of moles of Ag2CrO4 produced using the mole-to-mole ratio determined in Step 4.
Number of moles Ag2CrO4 = Number of moles AgNO3
Step 6: Substitute the value calculated in Step 3 into Step 5 to find the final answer.
Number of moles Ag2CrO4 = Number of moles AgNO3 = 146 g / 169.87 g/mol
Follow these calculations to find the exact number of moles of silver chromate produced from 146 g of silver nitrate.
I don't know but if all of the Ag in AgNO3 is converted to Ag2CrO4, then
1 mol 2AgNO3 = 1 mol Ag2CrO4; therefore, 1 mol AgNO3 will produce 1/2 mol Ag2CrO4. You have mols AgNO3 = 146/molar mass AgNO3 = approx 0.86 but that's an estimate.
Then 0.86 mols AgNO3 = 0.43 mols Ag2CrO4.
You need to redo all of the steps and get accuate numbers.