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wolverine [178]
3 years ago
5

The amount of pyridoxine (in grams) in a multiple vitamin is normally distributed with mean = 110 grams and standard deviation =

25 grams. What is the probability that a randomly selected vitamin will contain between 82 and 100 grams of pyridoxine?
Chemistry
1 answer:
KIM [24]3 years ago
5 0

Answer:

0.21108

Explanation:

Given,

Mean,

\mu = 110\text{ gram}

Standard deviation,

\sigma = 25\text{ gram}

Let X represents the amount of pyridoxine contained by vitamin,

So, the probability of vitamin will contain between 82 and 100 grams of pyridoxine,

= P( 82 ≤ X ≤ 100 )

P(\frac{82-\mu}{\sigma}\leq \frac{X-\mu}{\sigma}\leq \frac{100-\mu}{\sigma})

P(\frac{82 - 110}{25}\leq z \leq \frac{100-110}{25})

P(-1.12\leq z\leq -0.4)

P(z\leq -0.4)-P(z\leq -1.12)

=0.34458-0.13350

= 0.21108

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Solve the question that follows using the equation for the conversion of Celsius to Fahrenheit. F=95(C)+32 On February 9, 1934,
ahrayia [7]

Answer:

Buffalo, NY was colder on February 9, 1934

Explanation:

Temperature is the measure of thermal energy present in a given substance. It is a physical property of a matter which can be measured on the Celsius scale (°C), Fahrenheit scale (°F), and Kelvin scale (K).

<u>To convert Celsius (°C) to Fahrenheit (°F), we use the equation:</u>

°F = 9/5 (°C) + 32

Given: On February 9, 1934,

Temperature in Buffalo, NY: T₁ = (- 29) °C

Temperature in Anchorage, AL: T₂ = 19 °F

<u>To convert T₁ from °C to °F:</u>

9/5 (- 29 °C) + 32 = (- 52.2) + 32 = (- 20.2) °F

So,

Temperature in Buffalo, NY: T₁ = (- 20.2) °F

Temperature in Anchorage, AL: T₂ = 19 °F

⇒ T₁ < T₂

<u>Therefore, Buffalo, NY was colder on February 9, 1934.</u>

4 0
3 years ago
About the instruction that marko gave to hinano
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Explanation:

3 0
2 years ago
Dr. I. M. A. Brightguy adds 0.1727 g of an unknown gas to a 125-mL flask. If Dr. B finds the pressure to be 736 torr at 20.0°C,
AlladinOne [14]

Answer:

The gas that Dr. Brightguy added was O₂

Explanation:

Ideal Gases Law to solve this:

P . V = n . R . T

Firstly, let's convert 736 Torr in atm

736 Torr is atmospheric pressure = 1 atm

20°C = 273 + 20 = 293 T°K

125 mL = 0.125L

0.125 L . 1 atm = n . 0.082 L.atm / mol.K . 293K

(0.125L .1atm) / (0.082 mol.K /L.atm . 293K) = n

5.20x10⁻³ mol = n

mass / mol = molar mass

0.1727 g / 5.20x10⁻³ mol = 33.2 g/m

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Shalnov [3]
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Read 2 more answers
Calculate the rate constant at 200.°C for a reaction that has a rate constant of 8.30 × 10−4 s−1 at 90.°C and an activation ener
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Answer:

23.0 s⁻¹ is rate constant

Explanation:

Using the Arrhenius equation:

k = A * e^(-Ea/RT)

Where k is rate constant

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R is gas constant (8.314J/molK)

And T is absolute temperature (24°C + 273 = 297K)

Replacing:

k = 1.5x10¹¹s⁻¹ * e^(-55800J/mol/8.314J/molK*297K)

k = 1.5x10¹¹s⁻¹ * 1.53x10⁻¹⁰

k = 23.0 s⁻¹ is rate constant    i hope this helpsss

Explanation:

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