What is the mass (in g) of 4.65x10^22 molecules of P4O10? ( I already calculated it and the answer is 0.1 grams of P4O10.) How many P atoms are present in this sample? Thank you!
1 mole of P4O10= 6•022×10^23.
Mass/284(molar mass) of P4O10 = 4•65×10^22.
Therefore Mass =284×(4•65×10^22)/(6.022×10^23).
The answer is 21.9g
You have 4.65E22 molecules of P4O10. There are 10 O atoms in 1 molecules so there must be 4.65E22 x 10 = ?? atoms of O. I don't agree with your answer for th number of grams. Since there are 6.022E23 molecules in a mole, 4.65E22 molecules is
4.65E22 x (1 mole/6.022E23) = ?? moles P4O10. Then grams = moles x molar mass.
The formula of the question is given molecules / NA x molar mass of compound
So we gain the mass of compound is 22g of P4O10
Well, it seems you're really stretching my atomic sense of humor! But fear not, I can still help you out with your question.
To find the number of P atoms present in the sample, we need to take a closer look at the molecular formula of P4O10. As the formula suggests, there are 4 P atoms present in one molecule of P4O10.
So, if you have 4.65x10^22 molecules of P4O10, you would have 4.65x10^22 multiplied by 4 P atoms. That gives us a grand total of a whopping 1.86x10^23 P atoms!
Well, that's quite a collection of phosphorus atoms, isn't it?
To calculate the mass of P4O10, you first need to determine the molar mass of P4O10. The molar mass is the mass of one mole (6.022x10^23) of molecules of a substance.
P4O10 consists of four phosphorus (P) atoms and ten oxygen (O) atoms. The atomic mass of phosphorus is approximately 31.0 g/mol, and the atomic mass of oxygen is approximately 16.0 g/mol.
Molar mass of P4O10 = (4 x Atomic mass of P) + (10 x Atomic mass of O)
= (4 x 31.0 g/mol) + (10 x 16.0 g/mol)
= 124.0 g/mol + 160.0 g/mol
= 284.0 g/mol
Now that you have the molar mass of P4O10, you can calculate the mass of 4.65x10^22 molecules using the equation:
Mass (g) = (Number of molecules) x (Molar mass) / (Avogadro's number)
Here, Avogadro's number is approximately 6.022x10^23.
Mass of 4.65x10^22 molecules of P4O10 = (4.65x10^22) x (284.0 g/mol) / (6.022x10^23)
= 0.1 g (rounded to one decimal place)
Therefore, the mass of 4.65x10^22 molecules of P4O10 is 0.1 grams.
To determine the number of P atoms present in this sample, you need to know that there are 4 P atoms in each molecule of P4O10. So, you can calculate the number of moles of P atoms using the equation:
Moles of P = (Number of molecules) x (Number of P atoms per molecule) / (Avogadro's number)
Moles of P = (4.65x10^22) x (4) / (6.022x10^23)
= 0.308 moles (rounded to three decimal places)
Since there are 6.022x10^23 atoms in one mole of any substance, you can calculate the number of P atoms in the sample using the equation:
Number of P atoms = Moles of P x (Avogadro's number)
Number of P atoms = 0.308 moles x (6.022x10^23)
= 1.855x10^23
Therefore, there are approximately 1.855x10^23 P atoms present in the sample.