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tigry1 [53]
4 years ago
9

Which situation has the greatest pressure? A. Atmospheric pressure at sea level, equal to 1.01 X 105 N/m2 B. The pressure that a

person of mass 70 kg exerts on the floor when she balances on the ball of one foot, with an area of contact of 50 cm2 C. The pressure that a physics textbook of mass 2.5 kg exerts on a desk when it is lying flat on the desk, with an area of contact of 22 cm X 28 cm
(a) Identify the empirical formula of this compound.
Chemistry
1 answer:
Deffense [45]4 years ago
8 0

Answer:

B

Explanation:

We are given that

A.Atmospheric pressure=P_0=1.01\times 10^5N/m^2

B.Mass,m=70 kg

Area,A=50 cm^2=50\times 10^{-4} m^2

1 m^2=10^4 cm^2

Force=mg

Where g=9.8 m/s^2

Using the formula

F=70\times 9.8=686 N

P=\frac{F}{A}=\frac{686}{50\times 10^{-4}}=1.37\times 10^5 N/m^2

C.Mass ,m=2.5 kg

Area,A=22\times 28=616 cm^2=616\times 10^{-4} m^2

Pressure=\frac{mg}{A}=\frac{2.5\times 9.8}{616\times 10^{-4}}=397.7 N/m^2

In situation B has greatest pressure.

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Trimix 10/50 is a gas mixture that contians 10% oxygen and 50% helium, and the rest is nitrogen. If a tank of trimix 10/50 has a
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Answer: 1.61 x 10⁴ kPa

Dalton's law <u>states that the sum of the partial pressures of each gas equals the total pressure of the gas mixture.</u> According to this law,

Pi = xi P

where Pi is the partial pressure of the gas i, xi is the mole fraction of the gas i in the gas mixture and P is the total pressure.

The mole fraction <u>is defined as the quotient between the moles of solute (ni) and the total moles of the mixture (nt)</u>, which is calculated by adding the moles of all its components:

xi = \frac{n_{i} }{n_{t} }

In the Trimix 10/50 mix you have 10% oxygen, 50% helium and 40% nitrogen.

To calculate the total number of moles of the mixture and thus determine the molar fraction of helium, we consider 100 g and calculate the number of moles that represent 10 g of O₂ (n₁), 50 g of He (n₂) and 40 g of N₂ (n₃):

n₁ =  10 g x \frac{1 mol}{31.998 g} = 0.313 mol

n₂ =  50 g x \frac{1 mol}{8.005 g} = 6.246 mol

n₃ =  40 g x \frac{1 mol}{28.013 g} = 1.428 mol

Then the total number of moles (nt) will be:

nt = n₁ + n₂ + n₃ = 0.313 mol + 6.246 mol +1.428 mol

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and the partial pressure of helium in the mixture, according to Dalton's law, will be:

P₂ = x₂ P = 0.78 x 2.07 x 10⁴ kPa

P₂= 1.61 x 10⁴ kPa

So, <u>the partial pressure of helium if a tank of trimix 10/50 has a total pressure of 2.07 x 104 kPa is  1.61 x 10⁴ kPa</u>

5 0
3 years ago
construct the lewis structure of oo . draw the structure by placing atoms on the grid and connecting them with bonds. include al
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In Lewis dot structures, you draw the atom in the center and then surround the atom with its valence electrons. The Lewis structure for O is as shown in the attached diagram.

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