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Kryger [21]
3 years ago
9

a sample of air occupies 2.50 L at a temperature of 22.0c . what volume will this sample will this occupy inside a hot air baloo

n at a temperature of 43.0c assume that the pressure inside the balloon remains constant.
Chemistry
2 answers:
Zinaida [17]3 years ago
8 0

Answer:

The volume occupied by the air inside the hot balloon is 2.67 L.

Explanation:

Initial volume of the balloon =V_1= 2.50 L

Initial temperature of the air inside the balloon T_1= 22.0 °C = 295 K

Final volume of the balloon = V_2

Final temperature of the air inside the balloon =T_2= 43.0 °C = 316 K

Using Charles law:

\frac{V_1}{T_1}=\frac{V_2}{T_2}

V_2=\frac{V_1\times T_2}{T_1}=\frac{2.50 L\times 316 K}{295 K}=2.67 L

The volume occupied by the air inside the hot balloon is 2.67 L.

rosijanka [135]3 years ago
6 0
V1/T1= V2/T2   V =volume T= temp (in kelvin unit) 

2.5/(22+273)=V2/(43+273)
V2=2.7L
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Answer:

I think it's A

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3 years ago
Propane(C3H8) combusts with oxygen gas. If you start with 15 grams of Propane, how many grams of carbon dioxide will be produced
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<em>mC₃H₈: 44 g/mol</em>
<em>mCO₂: 44 g/mol</em>
---------------------

C₃H₈ + 5O₂ ----> 3CO₂ + 4H₂O
44g                    (44·3)g


44g C₃H₈ ------ 132g CO₂
15g C₃H₈ ------ X
X = (15×132)/44
<u>X = 45g CO₂
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4 0
3 years ago
3. Give an example of how carbon is transferred frem being in a living to a non-living<br> organism.
slavikrds [6]

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Carbon moves from living things to the atmosphere. Each time you exhale, you are releasing carbon dioxide gas (CO2) into the atmosphere. Animals and plants need to get rid of carbon dioxide gas through a process called respiration. Carbon moves from fossil fuels to the atmosphere when fuels are burned.

4 0
3 years ago
What is the percentage composition when 10g of magnesium combines with 4g of nitrogen?
Ivanshal [37]
The %  composition   when 10g of magnesium combine   with  4g of   nitrogen  is  71.43%   magnesium   and  28.57 %  nitrogen

               calculation

%
  composition  =  mass  of an element  / total mass  x100
mass  of magnesium = 10 g
mass of nitrogen  =  4g

calculate  the  total  mass  used

=  10g of  Magnesium  + 4 g of  nitrogen = 14 grams

%   composition for  magnesium  is therefore  =  10/14  x100 = 71.43 %

%  
composition  for  nitrogen  is therefore = 4 /14  x100  =   28.57 %
7 0
3 years ago
How many particles are in 23 g of H 2 O?
Sedaia [141]
1 mole of any substance contains 6.022 × 1023 particles.

⚛ 6.022 × 1023 is known as the Avogadro Number or Avogadro Constant and is given the symbol NA

N = n × NA

· N = number of particles in the substance

· n = amount of substance in moles (mol)

· NA = Avogardro Number = 6.022 × 10^23 particles mol-1


For H2O we have:

2 H at 1.0 each = 2.0 amu
1 O at 16.0 each = 16.0 amu
Total for H2O = 18.0 amu, or grams/mole

It takes 18 grams of H2O to obtain 1 mole, or 6.02 x 1023 molecules of water. Think about that before we answer the question. We have 25.0 grams of water, so we have more than one mole of water molecules. To find the exact number, divide the available mass (25.0g) by the molar mass (18.0g/mole). Watch how the units work out. The grams cancel and moles moves to the top, leaving moles of water. [g/(g/mole) = moles].

Here we have 25.0 g/(18.0g/mole) = 1.39 moles water (3 sig figs).

Multiply 1.39 moles times the definition of a mole to arrive at the actual number of water molecules:

1.39 (moles water) * 6.02 x 1023 molecules water/(mole water) = 8.36 x 1023 molecules water.

That's slightly above Avogadro's number, which is what we expected. Keeping the units in the calculations is annoying, I know, but it helps guide the operations and if you wind up with the unit desired, there is a good chance you've done the problem correctly.

N = n × (6.022 × 10^23)


1 grams H2O is equal to 0.055508435061792 mol.

Then 23 g of H2O is 1.2767 mol


To calculate the number of particles, N, in a substance:

N = n × NA

N = 1.2767 × (6.022 × 10^23)

N= 176.26

N=
3 0
2 years ago
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