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VMariaS [17]
3 years ago
6

Will mark brainliest if answered fast enough.

Chemistry
2 answers:
MrRa [10]3 years ago
6 0

Answer:

1,3,5,6

Explanation:

I took the test

stepan [7]3 years ago
3 0

Answer:

the answer is 1,3,5 and 6 :)

Explanation:

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Why is PCL3 called phosphorus chloride
Softa [21]
From your notation, it is phosphorus trichloride. Basically, there are three molecules of phosphorus chloride.
3 0
3 years ago
Which of the following is not present in an atom?<br> Electron<br> Element<br> Neutron<br> Proton
Licemer1 [7]

Answer:

an element is not in an atom

Explanation:

because the only things in a atom are electrons neutrons and protons

4 0
3 years ago
Read 2 more answers
8. A 220 mL sample of helium gas is in a cylinder with a movable piston at 105 kPa and 275K. The piston
Harrizon [31]

The sample has a new pressure of 274kPa. If at 105 kPa and 275K, a 220 mL sample of helium gas is contained in a cylinder with a moving piston. The sample is pushed till it has a 95.0 mL volume and 310K .

The macroscopic characteristics of ideal gases are related by the ideal gas law (PV = nRT). A gas is considered to be perfect if its particles (a) do not interact with one another and (b) occupy no space (have no volume). Where P= pressure  V= volume and T = temperature.

From ideal gas equation

P₁V₁/T₁ =P₂V₂/T₂

105×220÷275 = P₂ ×95÷310

P₂= (105×220×310)÷(275×95)

P2= 7161000/26125

P2 = 274.105 kPa

Hence, the new pressure of helium gas is 274kPa

To know more about Ideas gas equation

brainly.com/question/28837405

#SPJ1

8 0
1 year ago
How many moles of neon occupy a volume of 14.3 l at stp? how many moles of neon occupy a volume of 14.3 l at stp? 1.57 moles 0.6
andriy [413]
The  number   of  neon  moles  that  occupy  a volume of 14.3 l  at STP is calculated as follows

At STP 1  mole = 22.4 liters

what about  14.3 liters

by cross  multiplication
= (1 mole x 14.3 l)/22.4 l =0.638  moles  of  neon


5 0
3 years ago
Calculate the Molarity when a 6.11 mL solution of 0.1 H2SO4 is diluted with 105.12 mL of water
barxatty [35]

Molarity after dilution : 0.0058 M

<h3>Further explanation </h3>

The number of moles before and after dilution is the same  

The dilution formula

 M₁V₁=M₂V₂

M₁ = Molarity of the solution before dilution  

V₁ = volume of the solution before dilution  

M₂ = Molarity of the solution after dilution  

V₂ = Molarity volume of the solution after dilution

M₁=0.1 M

V₁=6.11

V₂=105.12

\tt M_2=\dfrac{M_1.V_1}{V_2}=\dfrac{0.1\times 6.11}{105.12}=0.0058~M

5 0
3 years ago
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