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rusak2 [61]
3 years ago
11

Inquiry Extension Consider a reaction that occurs between solid potassium and chlorine gas. If you start with an initial mass of

15.20 g K, and an initial mass of 2.830 g Cl2, calculate which reactant is limiting. Explain how to determine how much more of the limiting reactant would be needed to completely consume the excess reactant. Verify your explanation with an example
Chemistry
1 answer:
djyliett [7]3 years ago
5 0

Answer:

5 this is the answer call me brainy please

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2 years ago
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What is the daughter nuclide when 0-15 experiences positron emission?
Helen [10]

The daughter isotope (a decay product)of O-15 = N-15(Nitrogen 15)

<h3>Further explanation </h3>

Radioactivity is the process of unstable isotopes to stable isotopes by decay, by emitting certain particles,  

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Reaction

 \tt _8^{15}O\Rightarrow _7^{15}N+_1^0e

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5 0
2 years ago
A sample of gas occupies a volume of 445 mL at a temperature of 274 K. At what temperature will this sample of gas occupy a volu
Ksenya-84 [330]
V1 = 445ml V2 = 499ml
T1 = 274 K T2 = ?

By Charles Law,
V1/T1 = V2/T2
445/274 = 499/T2
By solving we get,
T2 = 307.25 K
4 0
2 years ago
If 0.600mol of chloride gas reacted with 0.500mol of aluminium metal to produce aluminium chloride,which reactant is in excess?h
alisha [4.7K]

Answer:

собак гандонов в гавне))))))))))

Explanation:

hloride,which reactant is in excess?how many moles of aluminium chloride can be produced during the reaction.hloride,which reactant is in excess?how many moles of aluсиськижопыссиськасуксиськипись loride can be produced during the reaction.hloride,which reactant is in excess?how many moles of aluminium chloride can be produced during the reaction.hloride,whichйух reactant is in excess?how many moles of aluminium chloride can be produced during the reaction.

5 0
2 years ago
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