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MakcuM [25]
3 years ago
10

Hydrazine (N2H4) emits a large quantity of

Chemistry
1 answer:
azamat3 years ago
5 0

Answer:

              1.75 moles of H₂O

Solution:

The Balance Chemical Equation is as follow,

                                   N₂H₄  +  O₂    →    N₂  +  2 H₂O

Step 1: Calculate the Limiting Reagent,

According to Balance equation,

             32.04 g (1 mol) N₂H₄ reacts with  =  32 g (1 mol) of O₂

So,

                   28 g of N₂H₄ will react with  =  X g of O₂

Solving for X,

                       X  =  (28 g × 32 g) ÷ 32.04 g

                       X  =  27.96 g of O₂

It means 29 g of N₂H₄ requires 47.96 g of O₂, while we are provided with 73 g of O₂ which is in excess. Therefore, N₂H₄ is the limiting reagent and will control the yield of products.

Step 2: Calculate moles of Water produced,

According to equation,

            32.04 g (1 mol) of N₂H₄ produces  =  2 moles of H₂O

So,

                        28 g of N₂H₄ will produce  =  X moles of H₂O

Solving for X,

                      X  =  (28 g × 2 mol) ÷ 32.04 g

                      X  =  1.75 moles of H₂O

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3 years ago
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A beaker with 155 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjug
OverLord2011 [107]

Answer:

ΔpH = 0.296

Explanation:

The equilibrium of acetic acid (CH₃COOH) in water is:

CH₃COOH ⇄ CH₃COO⁻ + H⁺

Henderson-Hasselbalch formula to find pH in a buffer is:

pH = pKa + log₁₀ [CH₃COO⁻] / [CH₃COOH]

Replacing with known values:

5.000 = 4.740 + log₁₀ [CH₃COO⁻] / [CH₃COOH]

0.260 =  log₁₀ [CH₃COO⁻] / [CH₃COOH]

1.820 = [CH₃COO⁻] / [CH₃COOH] <em>(1)</em>

As total molarity of buffer is 0.100M:

[CH₃COO⁻] + [CH₃COOH] = 0.100M <em>(2)</em>

Replacing (2) in (1):

1.820 = 0.100M - [CH₃COOH] / [CH₃COOH]

1.820[CH₃COOH] = 0.100M - [CH₃COOH]

2.820[CH₃COOH] = 0.100M

[CH₃COOH] = 0.100M / 2.820

[CH₃COOH] = <em>0.035M</em>

Thus: [CH₃COO⁻] = 0.100M - 0.035M = <em>0.065M</em>

5.40 mL of a 0.490 M HCl are:

0.0054L × (0.490mol / L) = 2.646x10⁻³ moles HCl.

Moles of CH₃COO⁻ are: 0.155L × (0.065mol / L) = 0.0101 moles

HCl reacts with CH₃COO⁻ thus:

HCl + CH₃COO⁻ → CH₃COOH

After reaction, moles of CH₃COO⁻ are:

0.0101 moles - 2.646x10⁻³ moles = <em>7.429x10⁻³ moles of CH₃COO⁻</em>

<em />

Moles of CH₃COOH  before reaction are: 0.155L × (0.035mol / L) = 5.425x10⁻³ moles of CH₃COOH. As reaction produce 2.646x10⁻³ moles of CH₃COOH, final moles are:

5.425x10⁻³ moles +  2.646x10⁻³ moles = <em>8.071x10⁻³ moles of CH₃COOH</em>. Replacing these values in Henderson-Hasselbalch formula:

pH = 4.740 + log₁₀ [7.429x10⁻³ moles] / [8.071x10⁻³ moles]

pH = 4.704

As initial pH was 5.000, change in pH is:

ΔpH = 5.000 - 4.740 = <em>0.296</em>

4 0
3 years ago
Kia is doing an experiment in science lab. She is given a beaker containing 100 g of liquid. The beaker has markings on the side
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7 0
3 years ago
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