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PSYCHO15rus [73]
3 years ago
8

At a particular temperature and [A]0 = 2.00 x 10-2 Molar, concentration versus time data were collected for this reaction and a

plot of ln[A]t versus time resulted in a straight line with a slope value of -2.97 x 10-2 min-1.
What is the half-life of this reaction?
Chemistry
1 answer:
madreJ [45]3 years ago
4 0
<h2>Answer:kllk<em>klkkkk</em></h2>

Explanation:

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What mass of F2 is needed to produce 180 g of PF3 if the reaction has a 78.1% yield?
nexus9112 [7]

Answer:

91.26 g

Explanation:

Given data:

Mass of PF₃ = 180 g

Mass of F₂ required = ?

Solution:

Chemical equation:

P₄ + 6F₂   → 4PF₃

Moles of PF₃:

Number of moles = mass/ molar mass

Number of moles = 180 g/ 88 g/mol

Number of moles = 2.05 mol

Now we will compare the moles of PF₃ with F₂.

                        PF₃            :           F₂

                          4               :           6

                          2.05         :           6/4×2.05 = 3.075

Mass of  F₂:

Mass of F₂ = moles × molar mass

Mass of F₂ = 3.075 mol × 38 g/mol

Mass of F₂ =  116.85 g

If reaction yield is 78.1%:

116.85 /100 ×78.1 = 91.26 g

6 0
3 years ago
Determine the resulting pH when 75 mL of 0.05M HBr is reacted with 74 mL of 0.075 M KOH
Sunny_sXe [5.5K]

Answer:

pH = 12.08

Explanation:

  • H⁺ + OH⁻ → H₂O

First we <u>calculate how many moles of each substance were added</u>, using <em>the given volume and concentration</em>:

  • HBr ⇒ 0.05 M * 75 mL = 3.75 mmol HBr
  • KOH ⇒ 0.075 M * 74 mL = 5.55 mmol KOH

As HBr is a strong acid, it dissociates completely into H⁺ and Br⁻ species. Conversely, KOH dissociates completely into OH⁻ and K⁺ species.

As there are more OH⁻ moles than H⁺ moles (5.55 vs 3.75), we <u>calculate how many OH⁻ moles remain after the reaction</u>:

  • 5.55 - 3.75 = 1.8 mmoles OH⁻

With that<em> number of moles and the volume of the mixture</em>, we <u>calculate [OH⁻]</u>:

  • [OH⁻] = 1.8 mmol / (75 mL + 74 mL) = 0.0121 M

With [OH⁻], we <u>calculate the pOH</u>:

  • pOH = -log[OH⁻] = 1.92

With the pOH, we <u>calculate the pH</u>:

  • pH = 14 - pOH
  • pH = 12.08
6 0
3 years ago
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