1.) what mass of zinc is needed to completely react with 4.00 g of silver nitrate?
2.) If excess ammonium sulfate reacts with 22.5 g of calcium hydroxide according to the following unbalanced chemical equation:
(NH4)2 SO4 + Ca (OH)2 → CaSO4 + NH3 + H2O
Now, how do I go from here?
Continue #2: So it says to : Calculate the mass of ammonia, NH3, that can be produced.
Can someone explain how to derive to the answer? Please
TEST VERY SOON
1.
Zn + 2AgNO3 ==> Zn(NO3)2 + 2Ag
mols AgNO3 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols AgNO3 to mols Zn.
Now convert mols Zn to grams Zn. g Zn = mols Zn x atomic mass Zn.
2. The balanced equation is as follows:
(NH4)2SO4 + Ca(OH)2 → CaSO4 + 2NH3 + 2H2O
mols Ca(OH)2 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Ca(OH)2 to mols NH3. Then convert mols NH3 to grams.
g NH3 = mols NH3 x molar mass NH3.
To solve these types of stoichiometry problems, you need to follow a step-by-step approach. I'll explain how to solve each question:
1.) What mass of zinc is needed to completely react with 4.00 g of silver nitrate?
Step 1: Write the balanced chemical equation.
The balanced equation for the reaction between zinc and silver nitrate is:
Zn + 2AgNO3 → Zn(NO3)2 + 2Ag
Step 2: Calculate the molar mass.
The molar mass of zinc is 65.38 g/mol, and the molar mass of AgNO3 is 169.87 g/mol.
Step 3: Convert the given mass of silver nitrate to moles.
To do this, use the formula:
moles = mass / molar mass
For 4.00 g of silver nitrate:
moles = 4.00 g / 169.87 g/mol
Step 4: Apply the stoichiometry ratio from the balanced equation.
From the balanced equation, we know that the ratio of Zn to AgNO3 is 1:2.
Step 5: Calculate the moles of zinc.
Multiply the moles of silver nitrate by the stoichiometry ratio:
moles of Zn = moles of AgNO3 / 2
Step 6: Convert moles of zinc to grams.
To do this, use the formula:
mass = moles x molar mass
Finally, calculate the mass of zinc:
mass of Zn = moles of Zn x molar mass of Zn
2.) If excess ammonium sulfate reacts with 22.5 g of calcium hydroxide according to:
(NH4)2 SO4 + Ca (OH)2 → CaSO4 + NH3 + H2O
Step 1: Write the balanced chemical equation.
The balanced equation is already given.
Step 2: Calculate the molar mass.
The molar mass of (NH4)2SO4 is 132.14 g/mol, and the molar mass of Ca(OH)2 is 74.09 g/mol.
Step 3: Convert the given mass of calcium hydroxide to moles.
To do this, use the formula:
moles = mass / molar mass
For 22.5 g of calcium hydroxide:
moles = 22.5 g / 74.09 g/mol
Step 4: Apply the stoichiometry ratio from the balanced equation.
From the balanced equation, we see that the ratio of (NH4)2SO4 to Ca(OH)2 is 1:1.
Step 5: Calculate the moles of (NH4)2SO4.
moles of (NH4)2SO4 = moles of Ca(OH)2
Step 6: Convert moles of (NH4)2SO4 to grams.
mass = moles x molar mass
Finally, calculate the mass of (NH4)2SO4:
mass of (NH4)2SO4 = moles of (NH4)2SO4 x molar mass of (NH4)2SO4
Follow these steps using the given information, and you'll be able to find the mass of zinc and (NH4)2SO4 needed in each respective question.