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Anastaziya [24]
3 years ago
15

a 40-lb container of peat moss measure 14x20x30 inches and has an average density of 0.13 g/cm^3. how many bags of peat moss are

needed to cover an area measure 1 3ft by 25 ft to a depth of 1.9 inches?
Chemistry
1 answer:
telo118 [61]3 years ago
4 0

Volume of the peat moss = 14\times 20\times 30 inches

= 8400 in^{3}

Convert the above volume into cm^{3}

1 in^{3}= 16.4 cm^{3}

Thus, volume in cm^{3} is:

Volume of peat moss =  8400 in^{3}\times \frac{16.4 cm^{3}}{1 in^{3}}

= 137760 cm^{3}

Now,

Total volume by using area and depth of the peat moss = area of peat moss \times depth of peat moss

= (13 ft \times  25 ft)\times 1.9 inches

= (325 ft^{2})\times 1.9 inches

Convert above values in cm to get the value of volume in cm^{3}:

1 ft= 30.48 cm

1 in= 2.54 cm

Thus, volume in cm^{3} is:

Total volume = (325 ft^{2}\times\frac{(30.48 cm)^{2}}{(1 ft)^{2}})\times (1.9 in\times \frac{2.54 cm}{1 in})

= 301934.88 cm^{2}\times 4.826 cm

= 1457137.73088 cm^{3}

Now, number of bags is calculated by the ratio of total volume of the peat moss to the volume of the peat moss.

Number of bags  =\frac{total volume of peat moss}{volume of peat moss}

Substitute the values of volume in above formula:

Number of bags  = \frac{1457137.73088 cm^{3}}{137760 cm^{3}}

= 10.57

≅ 11 bags

Thus, number of bags of peat moss are needed to cover an area measure 13 ft by 25 ft to a depth of 1.9 inches are 11 bags.


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Karo-lina-s [1.5K]

Answer:

I cannot give you all the answer but I can help you to solve those.

Explanation:

The first question:

How many grams are there in 7.5×10^{23} molecules of H_{2} SO_{4}?

So we need to find the molecular mass first, use your periodic table,

And then we can find out 2+32+16×4=98 g/mol

Then, we need to find how many moles, by using Avogadro's constant:

Avogadro's constant: 1 mole = 6.02×10^{23}

∴\frac{7.5*10^{23} }{6.02*10^{23}}=1.25 mol(2d.p.)

Lastly, find the grams using the formula M= \frac{m}{n}

m=Mn

m=1.25*98

m=122.5g

-------------------------------------------------------------------------------------------------------------

In conclusion, use those formula to help you:

M= \frac{m}{n} (which M = molecular mass(atomic mass) m=mass of the substance and n = moles)

Avogadro's constant: \frac {molecular mass} {6.02*10^{23}} = moles

5 0
3 years ago
I need an answer now please asap and you will me marked brainiest please it's missing I need it now.
kogti [31]

Answer:

Molecular Mass:

1. 40g per mole

2. 19g per mole

3. 64g per mole

4. 32 g per mole

5. 17g per mole

6. 59.5g per mole

7.58.5 g per mole

8.220g per mole

9. 78g per mole

10. 200g per mole

Explanation:

Molecular Mass = Number of atom x atomic mass of an element

Your Welcome~

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3 years ago
Consider the motion diagram. It illustrates a car's velocity (V) and acceleration (A). The BEST description of a car’s velocity
Masja [62]

Answer:

wheres the diagram ?

Explanation:

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Equal volumes of H2 and O2 are placed in a balloon and then ignited. Assuming that the reaction goes to completion, which gas wi
nirvana33 [79]

The reaction is

2H₂(g)  + O₂(g) ---> 2H₂O

Thus as per balanced equation two moles of hydrogen will react with one moles of oxygen.

There is a directly relation between moles and volume. [One mole of each gas occupies 22.4 L of volume at STP]

Thus we can say that two unit volume of hydrogen will react with one unit volume of oxygen

Now as we have started with equal units of volume of both oxygen and hydrogen, half of oxygen will be consumed against complete volume of hydrogen

so the gas which will remain in excess is oxygen

4 0
3 years ago
What is the density of an object that has a mass of 149. 8 g and displaces 12. 1 ml of water when placed in a graduated cylinder
kozerog [31]

Answer:

<h2>12.38 g/mL</h2>

Explanation:

The density of a substance can be found by using the formula

d =  \frac{m}{v}  \\

m is the mass

v is the volume

From the question

m = 149.8 g

v = 12.1 mL

We have

d =  \frac{149.8}{12.1}  = 12.380165... \\

We have the final answer as

<h3>12.38 g/mL</h3>

Hope this helps you

4 0
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