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denis23 [38]
3 years ago
10

The thermal decomposition of N2O5 obeys first-order kinetics. At 45°C, a plot of ln[N2O5] versus t gives a slope of −6.40 × 10−4

min−1. What is the half-life of the reaction?
Chemistry
1 answer:
finlep [7]3 years ago
5 0

Answer:

  • <u>1,080 min</u>

<u></u>

Explanation:

A <em>first order reaction</em> follows the law:

     rate=k[A]  , where [A] is the concentraion of the reactant A.

Equivalently:

       \dfrac{d[A]}{dt}=-k[A]

Integrating:

    \dfrac{d[A]}{[A]}=-kdt

   \ln \dfrac{[A]}{[A_o]}=-kt

Half-life means [A]/[A₀] = 1/2, t = t½:

  •    t½ = ln (2) / k

That means that the half-life is constant.

The slope of the plot of ln [N₂O₅]  is -k. Then k is equal to 6.40 × 10⁻⁴ min⁻¹.

Thus, you can calculate t½:

   t½ = ln(2) / 6.40 × 10⁻⁴ min⁻¹

   t½ = 1,083 min.

Rounding to 3 significant figures, that is 1,080 min.

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Helium gas diffuses 4 times as fast as an unknown gas. What is relative molecular mass of the gas​
Inessa05 [86]

The relative molecular mass of the gas​ : 64 g/mol

<h3>Further explanation</h3>

Given

Helium rate = 4x an unknown gas

Required

The relative molecular mass of the gas​

Solution

Graham's Law

\tt \dfrac{r_1}{r_2}=\sqrt{\dfrac{M_2}{M_1} }

r₁=4 x r₂

r₁ = Helium rate

r₂ = unknown gas rate

M₁= relative molecular mass of Helium = 4 g/mol

M₂ = relative molecular mass of the gas​

Input the value :

\tt \dfrac{4r_2}{r_2}=\sqrt{\dfrac{M_2}{4} }\\\\16=\dfrac{M_2}{4}\\\\M_2=64~g/mol

7 0
2 years ago
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Hope this helps~
8 0
3 years ago
CaC2 + 2H2O → C2H2 + Ca(OH)2 If 2.8 moles of CaC2 are consumed in this reaction, how many grams of H2O are needed?
Strike441 [17]

Answer:

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8 0
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1. Convert the following temperatures to K.<br> a) 104 C<br> b) -3 C
gogolik [260]

Answer:

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b) 270 k

Explanation:

a) 104 + 273 = 377 k

b) -3 + 273 = 270 k

3 0
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