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balandron [24]
3 years ago
12

Consider the following reaction:

Chemistry
1 answer:
adell [148]3 years ago
8 0

Answer:

1. d[H₂O₂]/dt = -6.6 × 10⁻³ mol·L⁻¹s⁻¹; d[H₂O]/dt = 6.6 × 10⁻³ mol·L⁻¹s⁻¹

2. 0.58 mol

Explanation:

1.Given ΔO₂/Δt…

    2H₂O₂     ⟶      2H₂O     +     O₂

-½d[H₂O₂]/dt = +½d[H₂O]/dt = d[O₂]/dt  

d[H₂O₂]/dt = -2d[O₂]/dt = -2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ = -6.6 × 10⁻³mol·L⁻¹s⁻¹

 d[H₂O]/dt =  2d[O₂]/dt =  2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ =  6.6 × 10⁻³mol·L⁻¹s⁻¹

2. Moles of O₂  

(a) Initial moles of H₂O₂

\text{Moles} = \text{1.5 L} \times \dfrac{\text{1.0 mol}}{\text{1 L}} = \text{1.5 mol }

(b) Final moles of H₂O₂

The concentration of H₂O₂ has dropped to 0.22 mol·L⁻¹.

\text{Moles} = \text{1.5 L} \times \dfrac{\text{0.22 mol}}{\text{1 L}} = \text{0.33 mol }

(c) Moles of H₂O₂ reacted

Moles reacted = 1.5 mol - 0.33 mol = 1.17 mol

(d) Moles of O₂ formed

\text{Moles of O}_{2} = \text{1.33 mol H$_{2}$O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{2 mol H$_{2}$O}_{2}} = \textbf{0.58 mol O}_{2}\\\\\text{The amount of oxygen formed is $\large \boxed{\textbf{0.58 mol}}$}

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Three complete orders on each side of the m=0 order can be produced in addition to the m = 0 order.

The ruling separation is

d=1 / (470mm −1) = 2.1×10⁻³ mm

Diffraction lines occur at angles θ such that dsinθ=mλ, where λ is the wavelength and m is an integer.

Notice that for a given order, the line associated with a long wavelength is produced at a greater angle than the line associated with a shorter wavelength.

We take λ to be the longest wavelength in the visible spectrum (538nm) and find the greatest integer value of m such that θ is less than 90°.

That is, find the greatest integer value of m for which mλ<d.

since  d / λ = 538×10⁻⁹m / 2.1×10 −6 m ≈ 3

that value is m=3.

There are three complete orders on each side of the m=0 order.

The second and third orders overlap.

Learn more about diffraction here : brainly.com/question/16749356

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How many moles of aluminum metal are required to produce 4.04 L of hydrogen gas at 1.11 atm and 27 °C by reaction with HCl? ​
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Answer:

0.121 moles of aluminum metal are required to produce 4.04 L of hydrogen gas at 1.11 atm and 27 °C by reaction with HCl

Explanation:

This is the reaction:

2 Al(s) + 6 HCl(aq) → 2 AlCl₃ (aq) + 3 H₂(g)

To make 3 moles of H₂, we need 2 moles of Al.

By conditions given, we will find out how many moles of H₂ do we have.

Let's use the Ideal Gas Law

P. V = n . R . T

1.11 atm . 4.04L = n . 0.082 L.atm/mol.K . 300K

(1.11 atm . 4.04L) / (0.082 mol.K/L.atm . 300K) = n

0.182 mol = n

So the rule of three will be:

If 3 moles of H₂ came from 2 moles of Al

0.182 moles of H₂ will come from x

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Who is telling what happens in Home Début?
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D

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Which type of reaction is Pb(NO3)2 + 2HCl → PbCl2 + 2HNO3?
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Answer:- D. Double- replacement reaction

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AB\rightarrow A+B

The given reaction looks different than this and so it is not decomposition reaction.

A single-replacement reaction looks like:

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Our reaction looks different from this so single-replacement is also not correct.

Synthesis reaction looks exactly opposite to decomposition reaction.

A+B\rightarrow AB

The given reaction is different than this and so it is not synthesis reaction also.

A double-replacement reaction looks like:

AB+CD\rightarrow AD+CB

In this reaction, the ions are exchanged as could be seen in the general reaction. On reaction side,A is with B and C is with D. On product side, A is with D and C is with B.

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