How many chloride ions are present in 1.7grams of magnesium chloride crystals?
mols MgCl2 = grams/molar mass = approx 0.02. There are 2 mols chloride ions per 1 mol MgCl2 so you have approx 0.04 mols Cl^-. There are 6.02E23 chloride ions in 1 mol so there must be ????? total chloride ions in 0.04 mols chloride ions.
I estimated the numbers; you should go through and recalculate all of the estimates.
What’s the answer
How many chloride ions are present in 1.7g of magnesium chloride crystals?
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Well, in order to find out how many chloride ions are present in 1.7 grams of magnesium chloride crystals, we need to do a little math.
First, we need to find the molar mass of magnesium chloride (MgCl2). Magnesium has a molar mass of 24.31 g/mol, and chlorine has a molar mass of 35.45 g/mol (since there are two chlorine atoms in magnesium chloride, we multiply the molar mass of chlorine by 2).
So, the molar mass of magnesium chloride is (24.31 + 2*(35.45)) g/mol = 95.21 g/mol.
Now, we can use the molar mass to determine the number of moles of magnesium chloride in 1.7 grams. We divide the mass by the molar mass:
1.7 g / 95.21 g/mol = 0.0178 mol.
Since magnesium chloride has 2 chloride ions for each molecule, we can multiply the number of moles by 2 to find the number of moles of chloride ions:
0.0178 mol * 2 = 0.0356 mol.
So, there are approximately 0.0356 moles of chloride ions in 1.7 grams of magnesium chloride crystals.
But remember, laughter is the best medicine, so keep those chloride ions laughing!
To determine the number of chloride ions present in 1.7 grams of magnesium chloride crystals, we need to use the concept of molar mass and Avogadro's number.
First, we need to find the molar mass of magnesium chloride (MgCl2) by summing the atomic masses of its constituent atoms. The atomic mass of magnesium (Mg) is 24.31 g/mol, and chlorine (Cl) has an atomic mass of 35.45 g/mol. Since there are two chloride ions in one magnesium chloride molecule, we multiply the atomic mass of chlorine by 2.
Molar mass of MgCl2 = (1 × atomic mass of magnesium) + (2 × atomic mass of chlorine)
= (1 × 24.31 g/mol) + (2 × 35.45 g/mol)
= 95.21 g/mol
Now we can calculate the number of moles of magnesium chloride using the formula:
moles = mass / molar mass
moles of MgCl2 = 1.7 g / 95.21 g/mol
= 0.0179 mol
Since magnesium chloride dissociates into Mg^2+ ions and two Cl− ions, the number of chloride ions is twice the number of moles of magnesium chloride.
Number of chloride ions = 2 × moles of MgCl2
= 2 × 0.0179 mol
= 0.0357 moles
Finally, we can calculate the number of chloride ions using Avogadro's number, which states that there are 6.022 × 10^23 particles (atoms, molecules, or ions) in one mole of any substance.
Number of chloride ions = moles × Avogadro's number
= 0.0357 mol × 6.022 × 10^23 ions/mol
Therefore, in 1.7 grams of magnesium chloride crystals, there are approximately 2.15 × 10^22 chloride ions.