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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)
What is A?

Couldn't wait so I got it wrong but for all the people needing this question answered the answer is A= 54.1

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 350 g Na what mass o class=
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Respuesta :

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

molar mass of Cl₂ is - 71.0 g/mol

number of Cl₂ moles are - 0.760 mol x 71.0 g/mol = 54.0 g

answer is 54.0 g of Cl₂ is needed

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