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Serggg [28]
3 years ago
15

The rate constant for the first-order decomposition of N2O5 (g) to NO2 (g) and O2 (g) is 7.48 * 10-3 s-1 at a given temperature.

Chemistry
1 answer:
alina1380 [7]3 years ago
8 0

Answer:

Explanation:

In this problem, we have a first-order decomposition reaction with a given rate constant. The rate law for a first-order reaction like this is

r

a

t

e

=

k

[

A

]

, where k is the rate constant and [A] is the concentration of the reactant (renamed as A, for brevity). To find the dynamics of the reaction with time, we can integrate the rate law to get an expression for [A](t):

rate = −d[A]dt = k[A]

[A]f =[A]i e−kt

We want the total pressure of the reaction chamber to be 0.145 atm, with a starting reactant pressure of 0.110 atm. To solve for the time this reaction takes, we need the reaction equation:

2N2O5(g) → 4NO2(g) + O2(g)

Using the stoichiometry of the reaction equation, we can determine the final pressure of the reactant. This requires us to rewrite the total pressure equation in terms of the change in pressure of the reactant.

Pf=0.145atm

Pi=0.110atm = pN2O5

iPf =pN2O5

f +pNO2 + pO2pNO2 = 4pO2

This comes from the stoichiometry.

pNO2 = 2(pN2O5i − pN2O5f )

This comes from the stoichiometry.

pNO2 = −2ΔpN2O5Pf = (pN2O5i + ΔpN2O5) − 2ΔpN2O 5 − 12ΔpN2O5

0.145atm =(0.110atm + ΔpN2O5) − 2.5ΔpN2O5 = 0.110atm − 1.5ΔpN2O5

ΔpN2O5 = −0.0233atm

pN2O5f = 0.110atm − 0.0233atm =

0.0867atm

This is our final pressure! Now we can use the integrated rate law.

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hco I believe

Explanation:

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How many moles are in 24.75 g of H2O? What is given the conversation and the unknown?
riadik2000 [5.3K]

Answer:

1.373 mol H₂O

General Formulas and Concepts:

<u>Chemistry - Atomic Structure</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis

Explanation:

<u>Step 1: Define</u>

24.75 g H₂O

<u>Step 2: Identify Conversions</u>

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol

<u>Step 3: Convert</u>

<u />24.75 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O} ) = 1.37347 mol H₂O

<u>Step 4: Check</u>

<em>We are given 4 sig figs. Follow sig fig rules and round.</em>

1.37347 mol H₂O ≈ 1.373 mol H₂O

7 0
2 years ago
An average bushel of apples has a mass of 10 kg and contains 5 dozen apples.
Alina [70]

Answer:

Average mass of 6 apple  = 1 kg

Explanation:

Given:

Average mass of 5 dozen apple = 10 kg

Find:

Average mass of 6 apple

Computation:

Average mass of 6 apple  = [Average mass of 1 apple] x [6 apple]

Average mass of 6 apple  = [10/(12 x 5)] x [6]

Average mass of 6 apple  = 1 kg

3 0
2 years ago
Approximately how many particles are in 2 moles?
schepotkina [342]

Answer:

1.2\times10^2^4 particles in 2 moles.

Explanation:

The number of particles that are contained in one mole, the international unit of amount of substance: by definition, exactly 6.022×10²³, and it is dimensionless. It is named after the scientist Amedeo Avogadro.

It is also known as Avogadro's constant.

∴ Number of particles in one mole = 6.022\times10^2^3

∴ Number of particles in 2 mole = 2 times Number of particles in one mole

∴ Number of particles in 2 mole=2\times6.022\times10^2^3=12.044\times10^2^3\approx1.2\times10^2^4

Hence there are 1.2\times10^2^4 particles in 2 moles.

4 0
2 years ago
Read 2 more answers
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