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Basile [38]
3 years ago
8

Determine the density of chlorine gas at 22C and 1.00 atm pressure

Chemistry
1 answer:
polet [3.4K]3 years ago
3 0
 <span>T = 22.0 + 273.15 =295.15 K 
Molar mass Cl2 = 70.906 g/mol 
d = molar mass x p / RT = 70.906 x 1.00 / 0.0821 x 295.15 = 2.93 g/L
Hope this isn't to much? If it doesn't help you know where to find me :)</span>
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How do plants affect the amount of carbon in Earth’s atmosphere?
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Answer:

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The atoms of Group 7A elements gain electrons when they form ions.<br><br> True<br> False
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Answer: True.

Explanation.

The group 7A is actually named group 17.

That group is the halogens: F, Cl, Br, I, At, and Ts (Ts is one of the last elements discovered).

Those elements have 7 valence electrons (notice that it is the same number as the second digit in 17).

The atoms with 7 valence electrons will "easily" gain one electron to get the configuration of the next noble gas (8 valence electrons). That is why these elements gain electrons to form ions.

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pentagon [3]
56% percent is the answer
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1.As with any grid, the periodic table has ________ (left to right) and __________ (up and down).
Inga [223]

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6 0
3 years ago
Carlos is making phosphorus trichloride using the equation below. He uses 15.5 g of phosphorus and collects 50.9 g of phosphorus
alex41 [277]

Answer: 35.4 g

Explanation:

The balanced reaction is :

2P+3Cl_2\rightarrow 2PCl_3

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of phosphorous}=\frac{15.5g}{31g/mol}=0.50moles

\text{Moles of phosphorous chloride}=\frac{50.9g}{137g/mol}=0.372moles

2P+3Cl_2\rightarrow 2PCl_3

According to stoichiometry :

2 moles of phosphorous chloride are produced by = 3 moles of Cl_2

Thus 0.37 moles of phosphorous chloride are produced by=\frac{3}{2}\times 0.372=0.558moles of Cl_2

Mass of Cl_2=moles\times {\text {Molar mass}}=0.558moles\times 71g/mol=35.4g

Thus 35.4 g of chlorine reacted with the phosphorus

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3 years ago
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