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grin007 [14]
3 years ago
12

Be sure to answer all parts. Nitrogen dioxide decomposes according to the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g) where Kp = 4.48 ×

10−13 at a certain temperature. If 0.65 atm of NO2 is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O2(g)?
Chemistry
1 answer:
AURORKA [14]3 years ago
5 0

Answer:

Partial Pressure of NO = 9.12 x 10^(-5)atm

Partial Pressure of O2 = 4.56 x 10^(-5)atm

Explanation:

2 NO2(g) ⇌ 2 NO(g) + O2(g)

Now,Kp = 4.48 × 10^(−13)

the initial pressure of NO2 that was added is 0.65 atm.

Now,

Partial pressure = mole fraction x total pressure

Let's say Total pressure is x;

So Partial pressure of (NO) = (1+1)x = 2x

Similarly Partial pressure of O2 = x

Now Kp =[(2x)² (x)] /[0.65]²

Since Kp = 4.48 × 10^(−13)

Thus, 4.48 × 10^(−13) =[(2x)² (x)] /[0.65]²

Multiply both sides by 0.65²

So, 4.48 x 0.65² x 10^(−13) = 2x³

2x³ = 1.899 x 10^(−13)

x³ =[ 1.889 x 10^(−13)] /2

= 0.945 x 10^(−13)

So x = ∛0.945 x 10^(−13) = 4.56 x 10^(-5)atm

So, Partial Pressure of NO = 2x = 2( 4.56 x 10^(-5)atm) = 9.12 x 10^(-5)atm

Also Partial Pressure of O2 = x = 4.56 x 10^(-5)atm

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Answer:

2.11 g hydrobromic acid (correct to 3SF)

Explanation:

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mass of C2H5BrO2 = 140.96g

Beginning with what we're given, 9.03*10^21 we then make a conversion by using Avegadro's number which is 6.02*10^23 per mole (Oct. 23 at 6:02 am is national mole day :) Then, we need to convert out of moles, 140.96g hydrombromic acid per mole.

It looks like this:

9.03*10^21 molecules • (1 mol C2H5BrO2 / 6.02*10^23 molecules) • (140g C2H5BrO2 / 1 mol) = 2.1144 g C2H5BrO2

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How many atoms are in 10.1 g Ne
LekaFEV [45]

Answer:

3.01 × 10²³ atoms Ne

General Formulas and Concepts:

<u>Atomic Structure</u>

  • Reading a Periodic Tables
  • Moles

<u>Stoichiometry</u>

  • Using Dimensional Analysis

Explanation:

<u>Step 1: Define</u>

<em>Identify</em>

[Given] 10.1 g Ne

[Solve] atoms Ne

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

Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

[PT] Molar Mass of Ne: 20.18 g/mol\

<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                       \displaystyle 10.1 \ g \ Ne(\frac{1 \ mol \ Ne}{20.18 \ g \ Ne})(\frac{6.022 \cdot 10^{23} \ atoms \ Ne}{1 \ mol \ Ne})
  2. [DA] Divide/Multiply [Cancel out units]:                                                          \displaystyle 3.01398 \cdot 10^{23} \ atoms \ Ne

<u>Step 4: Check</u>

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3.01398 × 10²³ atoms Ne ≈ 3.01 × 10²³ atoms Ne

4 0
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nikitadnepr [17]

Answer:

The limiting reagent is the O₂

Explanation:

We can think, this reaction

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Ratio between reactants is 2:1:1, 1:2:1, 1:1:2

For 2 mole of O₂, I need to react 1 mol of H₂ and 1 mol of S

0.187 mole of O₂, I need (the half)

0.093 mole of H₂ and 0.093 mole of S

For 1 mole of H₂, I need to react 2 mole of O₂ and 1 mol of S

2 mole of H₂, I need (the double of O₂ and the same for S)

4 mole of O₂ ; 2 mole of S

For 1 mol of S, I need to react 1 mol of H₂ and 2 mole of O₂

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