A chemist reacts sodium metal (Na) and chlorine gas (Cl) to form salt according to the balanced chemical equation: Na + Cl → NaCl. If the chemist has 35.0 g Na, what mass of chlorine must he or she use to react completely with the sodium? Finally, solve (remember significant figures):
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Answer:
The reaction involves adding Na and Cl₂ gas to form NaCl
since chlorine is a halogen it exists as a diatomic molecule - Cl₂
the balanced equation is
2Na + Cl₂ --> 2NaCl
the molar ratio reactants Na to Cl₂ is 2:1
the mass of Na present is 35.0 g
therefore number of moles of Na is - 35.0 g / 23 g/mol = 1.52 mol
according to the molar ratio , the number of Cl₂ moles required is half the number of Na moles present
If 2 moles of Na reacts with 1 mol of Cl₂
then 1.52 mol of Na reacts with - 1/2 x 1.52 mol = 0.760 mol of Cl₂
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Answer:
The answer is 54.1 on Edgenuity.
Explanation:
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