Consider the following reaction:
2NiS2+5O2--->2NiO+4SO2
a) How many moles of SO2 will be produced from 8.95 g of O2
b) How many grams of NiO would be formed from the reaction of 0.0125 mol of NiS2?
c) How many grams of O2 are needed to completely react with 3.74g of NiS2?
a) Well, to find out how many moles of SO2 will be produced from 8.95 g of O2, we need to do some math. But let's not get too serious here!
First, let's convert grams of O2 to moles. We can use the molar mass of O2 which is approximately 32 g/mol. So, 8.95 g of O2 is roughly 0.28 moles of O2.
Now, let's check the balanced equation. It tells us that for every 5 moles of O2, we get 4 moles of SO2. So, if we have 0.28 moles of O2, how many moles of SO2 will we get? Let's use a clownish equation setup:
0.28 mol O2 x 4 mol SO2 / 5 mol O2 = 0.224 mol SO2
So, approximately 0.224 moles of SO2 will be produced from 8.95 g of O2. Ta-dah!
b) Now, let's calculate how many grams of NiO will be formed from the reaction of 0.0125 mol of NiS2. Hold on to your clown noses!
According to the balanced equation, for every 2 moles of NiS2, we get 2 moles of NiO. So, if we have 0.0125 mol of NiS2, how many moles of NiO do we get? Let's do the math:
0.0125 mol NiS2 x 2 mol NiO / 2 mol NiS2 = 0.0125 mol NiO
Since we know the molar mass of NiO is approximately 74.7 g/mol, we can convert moles to grams. Ready for the finale?
0.0125 mol NiO x 74.7 g/mol NiO = 0.934 g NiO
So, approximately 0.934 grams of NiO would be formed from the reaction of 0.0125 mol of NiS2. Clown-tastic!
c) Lastly, let's find out how many grams of O2 are needed to react with 3.74 g of NiS2. Get your clown calculator ready!
First, let's convert grams of NiS2 to moles. The molar mass of NiS2 is approximately 90.76 g/mol. So, 3.74 g of NiS2 is about 0.0411 moles of NiS2.
Now, according to the balanced equation, for every 2 moles of NiS2, we need 5 moles of O2. So, if we have 0.0411 moles of NiS2, how many moles of O2 do we need? Let's find out:
0.0411 mol NiS2 x 5 mol O2 / 2 mol NiS2 = 0.10275 mol O2
Now, let's convert moles to grams. The molar mass of O2 is approximately 32 g/mol. Can you guess the grand finale weight?
0.10275 mol O2 x 32 g/mol O2 = 3.28 g O2
So, approximately 3.28 grams of O2 are needed to completely react with 3.74 g of NiS2. Clown makeovers for everybody!
a) To find the number of moles of SO2 produced from 8.95 g of O2, we need to use the molar ratio between O2 and SO2.
From the balanced equation, we can see that the molar ratio between O2 and SO2 is 5:4.
First, we need to convert the mass of O2 to moles using the molar mass of O2:
molar mass of O2 = 2 * molar mass of O = 2 * 16.00 g/mol = 32.00 g/mol
moles of O2 = mass of O2 / molar mass of O2
moles of O2 = 8.95 g / 32.00 g/mol = 0.280 mol
Now, using the molar ratio between O2 and SO2 (5:4), we can calculate the moles of SO2 produced:
moles of SO2 = moles of O2 * (4/5)
moles of SO2 = 0.280 mol * (4/5) = 0.224 mol
Therefore, 0.224 moles of SO2 will be produced from 8.95 g of O2.
b) To find the mass of NiO formed from the reaction of 0.0125 mol of NiS2, we need to use the molar ratio between NiS2 and NiO.
From the balanced equation, we can see that the molar ratio between NiS2 and NiO is 2:2.
moles of NiO = moles of NiS2
moles of NiO = 0.0125 mol
Now, we can calculate the mass of NiO formed using the molar mass of NiO:
molar mass of NiO = 58.69 g/mol
mass of NiO = moles of NiO * molar mass of NiO
mass of NiO = 0.0125 mol * 58.69 g/mol = 0.733 g
Therefore, 0.733 grams of NiO would be formed from the reaction of 0.0125 mol of NiS2.
c) To find the mass of O2 needed to completely react with 3.74 g of NiS2, we need to use the molar ratio between NiS2 and O2.
From the balanced equation, we can see that the molar ratio between NiS2 and O2 is 2:5.
First, we need to convert the mass of NiS2 to moles using the molar mass of NiS2:
molar mass of NiS2 = 58.71 g/mol
moles of NiS2 = mass of NiS2 / molar mass of NiS2
moles of NiS2 = 3.74 g / 58.71 g/mol = 0.0636 mol
Now, using the molar ratio between NiS2 and O2 (2:5), we can calculate the moles of O2 needed:
moles of O2 = moles of NiS2 * (5/2)
moles of O2 = 0.0636 mol * (5/2) = 0.159 mol
Finally, we can calculate the mass of O2 needed using the molar mass of O2:
molar mass of O2 = 32.00 g/mol
mass of O2 = moles of O2 * molar mass of O2
mass of O2 = 0.159 mol * 32.00 g/mol = 5.09 g
Therefore, 5.09 grams of O2 are needed to completely react with 3.74 g of NiS2.
To solve these problems, we will use the concept of stoichiometry, which relates the amounts of reactants and products in a chemical reaction. The balanced equation for the reaction is:
2NiS2 + 5O2 ---> 2NiO + 4SO2
a) To determine how many moles of SO2 will be produced from 8.95 g of O2, we need to convert the mass of O2 to moles using its molar mass and then apply the stoichiometry. Here's how you can solve it step by step:
1. Determine the molar mass of O2:
- The molar mass of O2 is 16.00 g/mol (since each oxygen atom has a molar mass of 16.00 g/mol, and there are two oxygen atoms in O2).
2. Convert the mass of O2 to moles:
- Divide the given mass of O2 (8.95 g) by its molar mass (16.00 g/mol):
8.95 g / 16.00 g/mol = 0.5594 mol O2
3. Apply the stoichiometry:
- According to the balanced equation, 5 moles of O2 produce 4 moles of SO2.
- Set up a ratio using the stoichiometric coefficients:
0.5594 mol O2 × (4 mol SO2 / 5 mol O2) = 0.4475 mol SO2
Therefore, 0.4475 moles of SO2 would be produced from 8.95 g of O2.
b) To determine how many grams of NiO would be formed from the reaction of 0.0125 mol of NiS2, we will again use stoichiometry. Here's how you can solve it:
1. Determine the molar mass of NiO:
- The molar mass of NiO is 74.71 g/mol (the molar mass of Ni is 58.69 g/mol, and the molar mass of O is 16.00 g/mol).
2. Apply the stoichiometry:
- According to the balanced equation, 2 moles of NiS2 produce 2 moles of NiO.
- Set up a ratio using the stoichiometric coefficients:
0.0125 mol NiS2 × (2 mol NiO / 2 mol NiS2) = 0.0125 mol NiO
3. Convert moles to grams:
- Multiply the number of moles of NiO by its molar mass:
0.0125 mol NiO × 74.71 g/mol = 0.9339 g NiO
Therefore, 0.9339 grams of NiO would be formed from the reaction of 0.0125 mol of NiS2.
c) To determine how many grams of O2 are needed to completely react with 3.74 g of NiS2, we will again use stoichiometry. Here's how you can solve it:
1. Determine the molar mass of NiS2:
- The molar mass of NiS2 is 90.76 g/mol (the molar mass of Ni is 58.69 g/mol, and the molar mass of S is 32.06 g/mol).
2. Convert the mass of NiS2 to moles:
- Divide the given mass of NiS2 (3.74 g) by its molar mass (90.76 g/mol):
3.74 g / 90.76 g/mol = 0.0411 mol NiS2
3. Apply the stoichiometry:
- According to the balanced equation, 2 moles of NiS2 require 5 moles of O2.
- Set up a ratio using the stoichiometric coefficients:
0.0411 mol NiS2 × (5 mol O2 / 2 mol NiS2) = 0.1028 mol O2
4. Convert moles to grams:
- Multiply the number of moles of O2 by its molar mass:
0.1028 mol O2 × 16.00 g/mol = 1.6448 g O2
Therefore, 1.6448 grams of O2 are needed to completely react with 3.74 g of NiS2.
First, there is no such thing as NiS2. NiS, perhaps, but not NiS2. However, the following answers are for the original question. I will show you how to do part a. The others are similar.
2NiS2+5O2--->2NiO+4SO2
How many mols O2 are in 8.95 g O2? That's mols = grams/molar mass = 8.95/32 = estimate 0.3 but you need to recalculate since this is an estimate.
Now look at the equation. 5 mols O2 will produce 4 moles SO2 so
0.3 mol O2 x (4 mols SO2/5 mols O2) = ? mols SO2 produced.