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irakobra [83]
3 years ago
12

how do I do this I’m confused

Chemistry
1 answer:
Naily [24]3 years ago
4 0

by using pro.gram..

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{\huge{\pink{\underline{\underline{❑❑❑❑❑❑❑❑❑~}}}}}

{\huge{\orange{\underline{\underline{﹌﹌﹌﹌﹌﹌﹌﹌﹌♪}}}}}

{\huge{\purple{\underline{\underline{✎﹏﹏﹏﹏﹏﹏﹏﹏﹏﹏}}}}}

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There are

2.52

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7 0
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Compound A is an organic compound which contains Carbon, Hydrogen and Oxygen. When 0.240g of the vapour of A is slowly passed ov
vesna_86 [32]

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hope it helpsss

4 0
4 years ago
A tarantula was walking along the sidewalk and walked 30 centimeters in 5 seconds. What was the average speed of the spider?
Marina CMI [18]
I’m pretty sure you would have to divide 5 and 30 and you will get 0.16666666 but I would think it would be 6cm/s but I could be wrong and if it is I’m am truly sorry.
7 0
3 years ago
Can someone help me with independent variables and dependant variables? I posted a question with the picture on it...please some
Naddik [55]

Answer:

independant=variable that has changed

dependant=variable affected by the change

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Explanation:

6 0
3 years ago
You are trying to determine the volume of the balloon needed to match the density of the air in the lab. You know that if you ca
vova2212 [387]
The equation to be used are:

PM = ρRT
PV = nRT
where
P is pressure, M is molar mass, ρ is density, R is universal gas constant (8.314 J/mol·K), T is absolute temperature, V is volume and n is number of moles

The density of air at 23.5°C, from literature, is 1.19035 kg/m³. Its molar mass is 0.029 kg/mol.

PM = ρRT
P(0.029 kg/mol) = (1.19035 kg/m³)(8.314 J/mol·K)(23.5+273 K)
P = 101,183.9 Pa

n = 0.587 g * 1 kg/1000 g * 1 mol/0.029 kg = 0.02024 mol
(101,183.9 Pa)V = (0.02024 mol)(8.314 J/mol·K)(23.5+273 K)
Solving for V,
V = 4.931×10⁻⁴ m³
Since 1 m³ = 1000 L
V = 4.931×10⁻⁴ m³ * 1000
V = 0.493 L

7 0
3 years ago
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