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son4ous [18]
3 years ago
12

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 24.0 g of carbon were burned in the presence of

82.7 g of oxygen, 18.7 g of oxygen remained unreacted. What mass of carbon dioxide was produced?
Chemistry
1 answer:
Novosadov [1.4K]3 years ago
8 0

Answer:

mass of CO2 = 88 g

Explanation:

It is stated in question that 18.7 g of oxygen remained unreacted which means that carbon is limiting reactant. Thus the amount of carbon dioxide produced depend upon the amount of carbon.

Given data:

mass of carbon = 24 g

total mass of oxygen 82.7 g

mass of unreacted oxygen = 18.7 g

mass of carbon dioxide = ?

Solution:

First of we will calculate the moles of carbon.

number of moles of carbon = mass of carbon / atomic weight

number of moles of carbon = 24 g/ 12 g/mol = 2 mol

Chemical equation:

C + O2 → CO2

now we compare the number of moles of carbon and carbon dioxide,

  C   :  CO2

  1    :    1

 2    :    2

Now we will calculate the mass of carbon dioxide from moles.

number of moles of CO2 = mass of CO2 / molar mass of CO2

2 mol × 44 g/mol = mass

mass of CO2 = 88 g

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Can someone help me with this molar mass problem?[It’s the last one]
quester [9]

Answer:

54.18 \times 10^{23} \ moles in 3 mole of  Al_2(SO_4)_3

Explanation:

It is clear that in the given 1\ mole of Al_2(SO_4)_3 have 3\ ions of SO_4^2^-

Therefore 3 moles of Al_2(SO_4)_3 will have 3\times3=9 \ ions of   SO_4^2^-

Since 1 ion of anything is equivalent to 6.02\times10^{23} \ moles

Therefore 3 moles of Al_2(SO_4)_3 will have 3\times3=9 \ ions of   SO_4^2^-

Which is equivalent to 9 \times6.02\times10^{23}=54.18\times10^{23} \ moles

Thus 3 moles of  Al_2(SO_4)_3 gives 54.18\times10^{23} \ moles of  SO_4^2^-.

5 0
3 years ago
What is the temperature of 0.645 mole of neon in a 2.00 L vessel at 4.68 atm?
storchak [24]

Answer:

—96.03°C

Explanation:

We'll begin by writing out the information provided by the question. This includes:

Number of mole (n) = 0.645 mole

Volume (V) = 2.00 L

Pressure (P) = 4.68 atm

Temperature (T) =?

Recall: that the gas constant = 0.082atm.L/Kmol

With the ideal gas equation PV = nRT, the temperature of the gas can be obtained as follow:

PV = nRT

4.68 x 2 = 0.645 x 0.082 x T

Divide both side 0.645 x 0.082

T = (4.68 x 2) /(0.645 x 0.082)

T = 176.97 K

Now, We can also express the temperature obtained in celsius as shown below:

Temperature (celsius) = temperature (Kelvin) - 273

Temperature (celsius) = 176.97 - 273

Temperature (celsius) = —96.03°C

The temperature of the Neon gas is

—96.03°C

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3 years ago
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I think the answer to this A but I’m not rlly sure
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How do we know stars are element factories?
djverab [1.8K]
In a nutshell, stars are mainly made of hygrogen, element 1.

over time, elements got more dense as they collided and cooled, leading to other gases, metals...

then they explode, which lead to all kinds of further complex elements.

The stuff that makes up the universe a lot of it is from exploding star stuff, and the Earth was built up upon these remains and the atoms that make up organisms even could originally be from stars.

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3 years ago
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