Elemental sulfur occurs as octatomic molecules, #S_8#. What mass (g) of fluorine gas is needed to react completely with 17.8 grams of sulfur to form sulfur hexafluoride?
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To calculate the mass of fluorine gas needed to react completely with 17.8 grams of sulfur to form sulfur hexafluoride, you first need to determine the molar mass of sulfur (S) and sulfur hexafluoride (SF6), then use stoichiometry to find the mass of fluorine required.
- The molar mass of sulfur (S) is 32.06 g/mol.
- The molar mass of sulfur hexafluoride (SF6) is 146.06 g/mol.
Using the stoichiometry of the reaction between sulfur and fluorine to form sulfur hexafluoride (SF6):
1 mole of S reacts with 6 moles of F2 to form 1 mole of SF6.
Now, we calculate the moles of sulfur (S) present in 17.8 grams:
moles of S = mass / molar mass = 17.8 g / 32.06 g/mol
Then, we use the stoichiometry to find the moles of fluorine gas (F2) required:
moles of F2 = moles of S * (6 moles F2 / 1 mole S)
Finally, we convert the moles of fluorine gas to grams using its molar mass:
mass of F2 = moles of F2 * molar mass of F2
Calculate and you'll get the mass of fluorine gas needed to react completely with 17.8 grams of sulfur to form sulfur hexafluoride.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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