How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen?
1 mole Ca(NO3)2 (the molar mass in grams) contains how many grams of oxygen? That will be 6*16 = 96 grams. Therefore,
164 g contains 96 g oxygen.
Set up a proportion and solve for g Ca(NO3)2 needed to obtain 24 g oxygen. Post your work if you get stuck.
To determine the number of grams of calcium nitrate that contain 24 grams of oxygen, we need to consider the molar ratios of calcium nitrate and oxygen in the compound.
The molar mass of calcium nitrate, Ca(NO3)2, can be calculated by summing the atomic masses of its constituent elements:
Ca: 1 atom x 40.08 g/mol = 40.08 g/mol
N: 2 atoms x 14.01 g/mol = 28.02 g/mol
O: 6 atoms x 16.00 g/mol = 96.00 g/mol
Adding these values gives the molar mass of calcium nitrate:
40.08 g/mol + 28.02 g/mol + 96.00 g/mol = 164.10 g/mol
Next, we need to find the molar mass of oxygen:
O: 1 atom x 16.00 g/mol = 16.00 g/mol
Now, we can determine the molar ratio of oxygen to calcium nitrate:
1 mole of Ca(NO3)2 contains 6 moles of oxygen (from the subscript 6 in the chemical formula).
To find the number of moles of oxygen in 24 grams, we use the molar mass of oxygen:
24 g / 16.00 g/mol = 1.5 moles
Since the molar ratio is 6 moles of oxygen to 1 mole of Ca(NO3)2, we divide the number of moles of oxygen by 6 to find the moles of calcium nitrate:
1.5 moles / 6 = 0.25 moles
Finally, we convert moles of calcium nitrate to grams using the molar mass of calcium nitrate:
0.25 moles x 164.10 g/mol = 41.025 grams
Therefore, 24 grams of oxygen is equivalent to approximately 41.025 grams of calcium nitrate.
To determine the number of grams of calcium nitrate (Ca(NO3)2) that contains 24 grams of oxygen, we need to calculate the molar mass of Ca(NO3)2 and the molar mass of oxygen.
The molar mass of Ca(NO3)2 is calculated by adding the atomic masses of calcium (Ca), nitrogen (N), and three oxygen (O) atoms:
Molar mass of Ca(NO3)2 = (atomic mass of Ca) + 2*(atomic mass of N) + 6*(atomic mass of O)
The atomic masses of calcium (Ca), nitrogen (N), and oxygen (O) are approximately 40.08 g/mol, 14.01 g/mol, and 16.00 g/mol, respectively.
Therefore, the molar mass of Ca(NO3)2 is:
Molar mass of Ca(NO3)2 = 40.08 + 2*(14.01) + 6*(16.00) g/mol
= 164.09 g/mol
Next, we need to determine the number of moles of oxygen in 24 grams. The molar mass of oxygen is approximately 16.00 g/mol, so the number of moles is calculated using the formula:
Number of moles = Mass / Molar mass
Number of moles of oxygen = 24 g / 16.00 g/mol
= 1.5 mol
Finally, we can use the mole ratio between oxygen and calcium nitrate to determine the amount of calcium nitrate that contains 1.5 moles of oxygen. From the balanced chemical equation,
2 moles of NO3^- (from Ca(NO3)2) react with 5 moles of O2 (from oxygen).
So, the mole ratio between oxygen (O2) and calcium nitrate (Ca(NO3)2) is:
5 mol O2 / 2 mol Ca(NO3)2
Converting 1.5 mol of oxygen to moles of calcium nitrate:
Number of moles of Ca(NO3)2 = (1.5 mol O2) * (2 mol Ca(NO3)2 / 5 mol O2)
= 0.6 mol Ca(NO3)2
Finally, we can calculate the mass of 0.6 moles of calcium nitrate using the equation:
Mass = Number of moles * Molar mass
Mass of Ca(NO3)2 = 0.6 mol * 164.09 g/mol
= 98.45 g
Therefore, 24 grams of oxygen is equivalent to approximately 98.45 grams of calcium nitrate (Ca(NO3)2).