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Step2247 [10]
3 years ago
8

The level of water in an olympic size swimming pool (50.0 meters long, 25.0 meters wide, and about 2.00 meters deep) needs to be

lowered 3.00 cm. If water is pumped out at a rate of 3.80 liters per second, how long will it take to lower the water level 3.00 cm?
Chemistry
1 answer:
MA_775_DIABLO [31]3 years ago
4 0

Initial dimension of the pool:

Length (L)= 50.0 m

Width (W)= 25.0 m

Depth (D) = 2.0 m

Initial Volume of the pool (V1)  = L*W*D = 50.0 * 25.0 *2.0 = 2500 m3

When the depth is lowered by 3 cm i.e. 0.03 m, the new depth becomes: 2.0 - 0.03 = 1.97 m

The new volume of the pool (V2) = 50.0*25.0*1.97 = 2462.5 m3

Volume of water to be pumped out = V1-V2 = 2500-2462.5 = 35.5 m3

Now, 1 m3 = 1000 L

therefore, 35.5 m3 == 35.5 *10^3 L

It is given that:

3.80 L of water is pumped out in 1 sec

Therefore, 35.5*10^3 L will be pumped out in:

= 1 s * 35.5*10^3 L/3.80 L = 9.34*10^3 sec



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goblinko [34]
Hey there! Great question;) Answer:It is neutrally charged, because it has the same number of electrons(negatively charged ions) and protons(positively charged ions) I hope this helps;)
6 0
3 years ago
An adult human lung has a volume of 2.9 liters. If its volume decreases to 1.2 liters and it contains 0.049 mole of air after it
Lera25 [3.4K]

Answer:

In full volume it contain 0.12 moles.

Explanation:

Given data:

Total volume= Vt = 2.9 L

Decreased volume= Vd = 1.2 L

Number of moles of air present in decreased volume= n = 0.049 mol

Number of moles of air in total volume= n = ?

Solution:

Formula:

Vt/ Vd = n (in total volume) /n ( decreased volume)

2.9 L / 1.2 L = X / 0.049 mol

2.42 = X / 0.049 mol

X = 2.42 × 0.049

X = 0.12 mol

6 0
3 years ago
A rock weighing 30.0 g is placed in a graduated cylinder displacing the volume from 22.3 mL to 27.6 mL. What is density of the r
cupoosta [38]
V'=v2-v1=27.6-22.3
density=mass/v'
ps: ml is the same as cubic cm
5 0
3 years ago
How many grams of chlorine gas react when 266.28 grams of aluminum reacts
erma4kov [3.2K]

Answer:

524.82 g Cl2

Explanation:

Balanced Equation:

2Al(s) + 3Cl(g) ⇒ 2AlCl (s)

Al: 26.982 g/mol     Cl: 35.453 g/mol

266.28g Al x 1mol Al/ 26.982g Al x 3mol Cl2/ 2mol Al x

35.453g Cl2/ 1mol Cl2 = 524.82 g Cl2

8 0
2 years ago
A chemist dissolves 716.mg of pure potassium hydroxide in enough water to make up 130.mL of solution. Calculate the pH of the so
Natasha_Volkova [10]

<u>Answer:</u> The pH of the solution is 13.0

<u>Explanation:</u>

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

Given mass of KOH = 716. mg = 0.716 g    (Conversion factor:  1 g = 1000 mg)

Molar mass of KOH = 56 g/mol

Volume of solution = 130 mL

Putting values in above equation, we get:

\text{Molarity of solution}=\frac{0.716\times 1000}{56g/mol\times 130}\\\\\text{Molarity of solution}=0.098M

1 mole of KOH produces 1 mole of hydroxide ions and 1 mole of potassium ions

  • To calculate hydroxide ion concentration of the solution, we use the equation:

pOH=-\log[OH^-]

We are given:

[tex[[OH^-]=0.098M[/tex]

Putting values in above equation, we get:

pOH=-\log(0.098)\\\\pOH=1.00

To calculate the pH of the solution, we use the equation:

pOH + pH = 14

So,  pH = 14 - 1.00 = 13.0

Hence, the pH of the solution is 13.0

4 0
3 years ago
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