How many atoms of tin are necessary to
react completely with 7.42 x 10(24th)g
of HF.
Sn(s) + 2HF(g) = SnF2(S) + H2 (g)
I think you must mean 7.42 x 10^24 molecules of HF, since I doubt that there are that many grams available.
since each atom of Sn reacts with 2 molecules of HF, it would require half as many Sn as HF.
To find out how many atoms of tin are necessary to react completely with a given amount of HF, we need to use stoichiometry and convert the mass of HF to the number of moles, then use the balanced chemical equation to determine the mole ratio between HF and Sn.
Let's follow these steps:
Step 1: Determine the molar mass of HF
The molar mass of HF is composed of hydrogen (H) with an atomic mass of approximately 1, and fluorine (F) with an atomic mass of approximately 19. So, the molar mass of HF is:
1(atomic mass of H) + 19(atomic mass of F) = 1 + 19 = 20 g/mol.
Step 2: Convert the given mass of HF to moles
To convert the mass (7.42 x 10^(24) g) of HF to moles, divide it by the molar mass of HF:
Number of moles of HF = Given mass of HF / Molar mass of HF
Number of moles of HF = (7.42 x 10^(24) g) / (20 g/mol) = 3.71 x 10^(23) mol.
Step 3: Use the balanced chemical equation to determine the mole ratio
From the balanced chemical equation, we can see that the mole ratio between HF and Sn is 2:1. This means that 2 moles of HF react with 1 mole of Sn.
Step 4: Calculate the number of moles of Sn required
Since the mole ratio between HF and Sn is 2:1, the number of moles of Sn required will be half of the number of moles of HF:
Number of moles of Sn = 1/2 * Number of moles of HF
Number of moles of Sn = 1/2 * 3.71 x 10^(23) mol = 1.855 x 10^(23) mol.
Step 5: Convert the number of moles of Sn to atoms
To convert the number of moles of Sn to atoms, use Avogadro's number, which is the number of atoms in one mole of any substance:
Number of atoms of Sn = Number of moles of Sn * Avogadro's number
Number of atoms of Sn = 1.855 x 10^(23) mol * (6.022 x 10^(23) atoms/mol)
Number of atoms of Sn = 1.116 x 10^(47) atoms.
Therefore, there are 1.116 x 10^(47) atoms of tin necessary to react completely with 7.42 x 10^(24) g of HF.