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leonid [27]
2 years ago
4

A bathtub is filling with water at a rate of 72 inch3/second. The density of water is 0.58 ounce/inch3. How long will it take fo

r the tub to fill with 11,000 ounces of water? Express your answer to the correct number of significant figures.
Chemistry
2 answers:
Roman55 [17]2 years ago
8 0
We can first find how much ounces it is filled per second:
72×0.58
=41.76ounces

We can then find how long it will take by dividing 11,000 by the abswer we found above:
11,000÷41.76
=263.4099...
≈263.41ounces

Therefore,the answer is 263.41 ounces.

Please also note that this question belongs to the mathematics category!

Hope it helps!
Archy [21]2 years ago
8 0

Answer: 263.4 sec

Explanation:

Ounces of water in 1 second = Density\times rate=0.58ounces/inch^3\times 72inch^3/sec=41.76ounces/ sec

This means that 41.76 ounces of water is getting collected in tub in 1 second

Then 11000 ounces of water will be collected in=\frac{1}{41.76}\times 11000=263.40seconds

The time taken to fill the tank upto 11000 ounces will 263.40 seconds.

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Is Plutonium an element, compound, solution* or heterogeneous mixture.
Blizzard [7]

Answer:

Its an element.

Explanation:

94 on the periodic table

8 0
2 years ago
How many grams of K2CO3 would you need to put on the spill to neutralize the acid according to the following equation? 2HBr(aq)+
Mkey [24]

Full Question:

A flask containing 420 Ml of 0.450 M HBr was accidentally knocked to the floor.?

How many grams of K2CO3 would you need to put on the spill to neutralize the acid according to the following equation?

2HBr(aq)+K2CO3(aq) ---> 2KBr(aq) + CO1(g) + H2O(l)

Answer:

13.1 g K2CO3 required to neutralize spill

Explanation:

2HBr(aq) + K2CO3(aq) → 2KBr(aq) + CO2(g) + H2O(l)

Number of moles = Volume * Molar Concentration

moles HBr= 0.42L x .45 M= 0.189 moles HBr

From the stoichiometry of the reaction;

1 mole of K2CO3 reacts  with 2 moles of HBr

1 mole = 2 mole

x mole = 0.189

x = 0.189 / 2 = 0.0945 moles

Mass = Number of moles * Molar mass

Mass = 0.0945 * 138.21  = 13.1 g

3 0
2 years ago
A 25.0 g sample of an alloy was heated to 100.0 oC and dropped into a beaker containing 90 grams of water at 25.32 oC. The tempe
elena55 [62]

Answer:

The specific heat of the alloy C_{a} = 0.37 \frac{KJ}{Kg K}

Explanation:

Mass of an alloy m_{a} = 25 gm

Initial temperature T_{a} = 100°c = 373 K

Mass of water m_{w} = 90 gm

Initial temperature of water T_{w} = 25.32 °c = 298.32 K

Final temperature T_{f} = 27.18 °c = 300.18 K

From energy balance equation

Heat lost by alloy = Heat gain by water

m_{a} C_{a}  [T_{a} - T_{f}] = m_{w} C_w (T_{f} -T_{w} )

25 × C_{a} × ( 373 - 300.18 ) = 90 × 4.2 (300.18 - 298.32)

C_{a} = 0.37 \frac{KJ}{Kg K}

This is the specific heat of the alloy.

4 0
2 years ago
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Reil [10]

Answer:

Not sure what the answer is

Explanation:

I did this a while ago and dont remember sorry

4 0
2 years ago
a compound contain 8.57g of carbon and 1.43g of hydrogen. The relative formula mass is 70 calculate the empirical formula of the
yanalaym [24]

Answer:

Empirical formula: CH2

Molecular formula: C5H10

5 0
1 year ago
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