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hram777 [196]
2 years ago
10

A bottle sitting on a table has no forces at all acting upon it.

Chemistry
2 answers:
solong [7]2 years ago
5 0

Answer:

I'm a bit confused on where the question is. Perhaps re-write it in the comments? I'd love to help but this seems more like an answer than a question xD

Explanation:

emmasim [6.3K]2 years ago
5 0

Answer:

Cool!

Explanation:

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What volume (ml) of fluorine gas is required to react with 1. 28 g of calcium bromide to form calcium fluoride and bromine gas a
Alexandra [31]

144 mL of fluorine gas is required to react with 1.28 g of calcium bromide to form calcium fluoride and bromine gas at STP.

<h3>What is Ideal Gas Law ? </h3>

The ideal gas law states that the pressure of gas is directly proportional to the volume and temperature of the gas.

PV = nRT

where,

P = Presure

V = Volume in liters

n = number of moles of gas

R = Ideal gas constant

T = temperature in Kelvin

Here,

P = 1 atm  [At STP]

R = 0.0821 atm.L/mol.K

T = 273 K  [At STP]

Now first find the number of moles

F₂  +  CaBr₂  →  CaF₂  +  Br₂

Here 1 mole of F₂ reacts with 1 mole of CaBr₂.

So,  199.89 g CaBr₂ reacts with  = 1 mole of F₂

1.28 g of CaBr₂ will react with = n mole of F₂

n = \frac{1.28\g \times 1\ \text{mole}}{199.89\ g}

n = 0.0064 mole

Now put the value in above equation we get

PV = nRT

1 atm × V = 0.0064 × 0.0821 atm.L/mol.K × 273 K

V = 0.1434 L

V ≈ 144 mL

Thus from the above conclusion we can say that 144 mL of fluorine gas is required to react with 1.28 g of calcium bromide to form calcium fluoride and bromine gas at STP.

Learn more about the Ideal Gas here: brainly.com/question/20348074

#SPJ4

4 0
1 year ago
A chemistry student needs of acetone for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student dis
galben [10]

Answer:

The answer is "7.90 \ g".

Explanation:

Please finds the complete question in the attached file.

Volume = 10.0 \ mL \\\\Density =0.79 g\  cm^3

\text{Density}=\frac{Mass}{Volume}

Mass = Density \times Volume

         =(0.790 g\ cm^3) \times 10.0 \ mL\\\\=7.90 \ g

The mass of acetone to be weighed is 7.90 \ g

8 0
2 years ago
How many moles of a gas would occupy 22.4 Liters at 273 K and 1 atm?
Molodets [167]

Answer:

1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm

Explanation:

An ideal gas is a set of atoms or molecules that move freely without interactions. The pressure exerted by the gas is due to the collisions of the molecules with the walls of the container. The ideal gas behavior is at low pressures, that is, at the limit of zero density. At high pressures the molecules interact and intermolecular forces cause the gas to deviate from ideality.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

  • P= 1 atm
  • V= 22.4 L
  • n= ?
  • R= 0.082 \frac{atm*L}{mol*K}
  • T=273 K

Reemplacing:

1 atm* 22.4 L= n* 0.082 \frac{atm*L}{mol*K} *273 K

Solving:

n=\frac{1 atm* 22.4 L}{0.082 \frac{atm*L}{mol*K} *273 K}

n= 1 mol

Another way to get the same result is by taking the STP conditions into account.

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C (or 273 K) are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

<u><em>1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm</em></u>

4 0
2 years ago
I need help with #3 name the compound
ioda
4-ethyl-3-methyl 1 hexane
4 0
3 years ago
Please help and thank you so much
olchik [2.2K]
A. Sorry if I’m wrong :(
8 0
2 years ago
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