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frosja888 [35]
3 years ago
8

How long does it take for 87.5 % of each isotope(Krypton-73, Krypton-74, Krypton-76, and Krypton-81) to decay?

Chemistry
1 answer:
fomenos3 years ago
3 0
1st half-life: 100%/2 = 50%
2nd half-life: 50%/2 = 25% + 50% (from first half-life)
3rd half-life: 25%/2 = 12.5% + 75% (from first and second half-lives

I looked it up...
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Answer:

32

Explanation:

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What is the tool used for measuring volume?
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4 0
3 years ago
Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) In
jek_recluse [69]

Answer: The percent yield of the reaction is 74 %

Explanation:

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

\text{Moles of aluminium}=\frac{2.5g}{27g/mol}=0.092mol

For oxygen gas:

\text{Moles of oxygen gas}=\frac{2.5g}{32g/mol}=0.078mol

The chemical equation for the reaction of titanium and chlorine gas follows:

4Al(s)+3O_2(g)\rightarrow 2Al_2O_3(s)

By Stoichiometry of the reaction:

4 moles of aluminium reacts with 3 moles of oxygen.

So, 0.092 moles of aluminium reacts with = \frac{3}{4}\times 0.092=0.069mol of oxygen

As, given amount of oxygen is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

4 moles of aluminium produce = 2 moles of Al_2O_3

So, 0.092 moles of aluminium will produce = \frac{2}{4}\times 0.092=0.046moles of Al_2O_3

Now, calculating the mass of aluminium oxide:

\text{Mass of aluminium oxide}=moles\times {\text {molar mas}}=0.046mol\times 102g/mol=4.7g

To calculate the percentage yield of titanium (IV) chloride, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield  = 3.5 g

Theoretical yield = 4.7 g

Putting values in above equation, we get:

\%\text{ yield of reaction}=\frac{3.5g}{4.7g}\times 100\\\\\% \text{yield of reaction}=74\%

Hence, the percent yield of the reaction is 74 %

6 0
3 years ago
ITS MY WORK FROM SCIENCE, AND I NEED THAT FOR NOW, I DONT EVEN KNOW HOW TO ANSWER THAT​
m_a_m_a [10]

Answer:

TEEHEE

Explanation:

5 0
3 years ago
Balance the following equation and determine the mole ratio of Cl2 to CCl4. CS2 + Cl2 CCl4 + S2Cl2
Andre45 [30]
CS₂ + Cl₂<span> </span>→ CCl₄ + S₂Cl₂<span> [unbalanced equation]

</span>CS₂ + 3Cl₂ → CCl₄ + S₂Cl₂ [balanced equation]

∴ the mole ratio of Cl₂ : CCl₄ is   3  :  1  (option D)
3 0
3 years ago
Read 2 more answers
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