2NiS2(s)+5O2(g)=2NiO(s)+4SO2(g)
1. how many kilograms of NiO would be formed from the reaction of .0125 mol of NiS2?
2. How many grams of O2 are needed to cmpletely react with 3.74 g of NiS2.
To solve these problems, we'll use the given balanced chemical equation:
2NiS2(s) + 5O2(g) → 2NiO(s) + 4SO2(g)
1. To find the amount of NiO formed from 0.0125 mol of NiS2, we need to use stoichiometry. According to the balanced equation, the mole ratio between NiS2 and NiO is 2:2 (from the coefficients in the equation).
0.0125 mol of NiS2 x (2 mol NiO / 2 mol NiS2) = 0.0125 mol NiO
Now, to find the mass of NiO formed, we need to multiply the moles by its molar mass. The molar mass of NiO is 74.69 g/mol.
0.0125 mol NiO x 74.69 g/mol = 0.934 g NiO
Therefore, 0.0125 mol of NiS2 would produce 0.934 g of NiO.
2. To find the mass of O2 needed to react with 3.74 g of NiS2, we'll again use stoichiometry. This time, we need to find the mole ratio between NiS2 and O2. From the balanced equation, the ratio is 2:5 (from the coefficients in the equation).
First, we need to convert the mass of NiS2 to moles:
3.74 g NiS2 x (1 mol NiS2 / 90.76 g NiS2) = 0.0412 mol NiS2
Now, based on the mole ratio, we can find the moles of O2 needed:
0.0412 mol NiS2 x (5 mol O2 / 2 mol NiS2) = 0.103 mol O2
Finally, to find the mass of O2, we'll multiply the moles by its molar mass. The molar mass of O2 is 32.00 g/mol.
0.103 mol O2 x 32.00 g/mol = 3.296 g O2
Therefore, 3.74 g of NiS2 would require 3.296 g of O2 to completely react.
To solve both of these questions, we will need to use stoichiometry and molar mass calculations. Stoichiometry is the study of the quantitative relationships between reactants and products in a chemical reaction.
1. How many kilograms of NiO would be formed from the reaction of 0.0125 mol of NiS2?
To calculate the mass of NiO formed, we need to know the molar mass of NiO. The molar mass of NiO is:
Ni: 58.69 g/mol
O: 16.00 g/mol
Molar mass of NiO = (Ni: 58.69 g/mol) + (O: 16.00 g/mol) = 74.69 g/mol
Now, using the given amount of NiS2 (0.0125 mol), we can use the stoichiometric coefficients from the balanced equation to find the molar ratio between NiS2 and NiO.
According to the balanced equation, 2 moles of NiS2 react to form 2 moles of NiO, so the molar ratio is 2:2.
Now, we can use the molar mass and the given mole amount (0.0125 mol) to calculate the mass of NiO formed.
Mass of NiO = Molar mass of NiO × moles of NiO
Mass of NiO = 74.69 g/mol × 0.0125 mol
Mass of NiO = 0.933625 g
To convert grams to kilograms, we divide by 1000:
Mass of NiO in kilograms = 0.933625 g ÷ 1000 = 0.000933625 kg
Therefore, 0.000933625 kg of NiO would be formed from the reaction of 0.0125 mol of NiS2.
2. How many grams of O2 are needed to completely react with 3.74 g of NiS2?
To calculate the amount of O2 required, we need to use the stoichiometry of the balanced equation.
First, we need to find the molar mass of NiS2:
Ni: 58.69 g/mol
S: 32.06 g/mol
Molar mass of NiS2 = (Ni: 58.69 g/mol) + (2 × S: 32.06 g/mol) = 122.81 g/mol
Using the given mass of NiS2 (3.74 g) and the molar mass of NiS2, we can calculate the moles of NiS2:
Moles of NiS2 = Mass of NiS2 ÷ Molar mass of NiS2
Moles of NiS2 = 3.74 g ÷ 122.81 g/mol
Next, we can use the stoichiometric coefficients from the balanced equation to determine the mole ratio between NiS2 and O2.
According to the balanced equation: 2 moles of NiS2 react with 5 moles of O2, so the mole ratio is 2:5.
Now, we can calculate the moles of O2 required:
Moles of O2 = Moles of NiS2 × (5 moles O2 / 2 moles NiS2)
Finally, we can convert the moles of O2 to grams using the molar mass of O2:
Mass of O2 = Moles of O2 × Molar mass of O2
Molar mass of O2 = 32.00 g/mol
Substituting the values into the equation:
Mass of O2 = Moles of O2 × 32.00 g/mol
Therefore, you can now calculate the grams of O2 needed to completely react with 3.74 g of NiS2 using the above formulas.
Convert 0.0125 mol NiS2 to mols NiO. That is 0.0125 mol NiS2 x (2 mol NiO/2 mol NiS2) = 0.0125 mol NiS2 x 2/2 = 0.0125 mol NiO.
Then g = mols NiO x molar mass NiO= ?
For part b convert g NiS2 to mols, convert that to mols O2 and that to grams O2. Follow the steps from part a.