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o-na [289]
3 years ago
10

A 35 L tank of oxygen is at 315 K with an internal pressure of 190 atmospheres. How

Chemistry
1 answer:
nata0808 [166]3 years ago
6 0

Answer:

600.7 moles

Explanation:

Applying,

PV = nRT................... Equation 1

Where P = Pressure of oxygen, V = Volume of oxygen, n = number of moles, R = molar gas constant, T = Temperature.

make n the subject of the equation

n = PV/RT............... Equation 2

From the question,

Given: P = 190 atm, V = 35 L, T = 135 K

Constant: R = 0.082 atm.dm³/K.mol

Substitute these values into equation 2

n = (190×35)/(135×0.082)

n = 600.7 moles of xygen

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Draw a basic atom (Bohr model showing me where everything is located in the above chart).
tino4ka555 [31]

Answer:

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Explanation:

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6 0
1 year ago
List a few ways that would lead you to believe a chemical reaction has occurred
iren2701 [21]
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Gas Production:
                         Some reactions proceed with the elimination of gas i.e. CO</span>₂ , H₂, N₂, H₂O e.t.c. 

Temperature Change:
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Thin Layer Chromatography:
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Instrumental Techniques:
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5 0
3 years ago
Write balanced complete ionic equation for the reaction AgNO3(aq)+KCl(aq)→AgCl(s)+KNO3(aq).
Nikitich [7]
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3 0
2 years ago
Read 2 more answers
Please help no links
jarptica [38.1K]

Answer:

23 L

Explanation:

We'll begin by converting celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 100 °C

Initial temperature (T₁) = 100 °C + 273

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 50.5 °C

Final temperature (T₂) = 50.5 °C + 273

Final temperature (T₂) = 323.5 K

Finally, we shall determine the initial volume of gas. This can be obtained as follow:

Initial temperature (T₁) = 373 K

Final temperature (T₂) = 323.5 K

Final volume (V₂) = 20 L

Initial volume (V₁) =?

V₁/T₁ = V₂/T₂

V₁ / 373 = 20 / 323.5

Cross multiply

V₁ × 323.5 = 373 × 20

V₁ × 323.5 = 7460

Divide both side by 323.5

V₁ = 7460 / 323.5

V₁ = 23 L

Thus, the original volume of the gas is 23 L

7 0
2 years ago
Indicate whether each of the statements below is true or false. Match the words in the left column to the appropriate blanks in
otez555 [7]

Answer:

1) ) CBr₄ has a higher boiling point than CCl₄: True

2 CBr₄ has weaker intermolecular forces than CCl₄: False

3) CBr₄ has a higher vapor pressure at the same temperature than CCl₄: False

4) CBr₄ is more volatile than CCl₄: False

Explanation:

1) ) CBr₄ has a higher boiling point than CCl₄: True :

Due to higher molecular weight CBr₄ has more london disperion forces thus making the intermolecular interactions stronger and thus it need more temperature to boil it off.

2 CBr₄ has weaker intermolecular forces than CCl₄: False

Due to higher molecular weight CBr₄ has more london disperion forces thus making the intermolecular interactions stronger.

3) CBr₄ has a higher vapor pressure at the same temperature than CCl₄: False

Due to higher molecular weight CBr₄ has more london disperion forces thus making the intermolecular interactions stronger. Thus the vapor pressure of it will be less than CCl₄ at the same temperature.

4) CBr₄ is more volatile than CCl₄: False

Due to higher molecular weight CBr₄ has more london disperion forces thus making the intermolecular interactions stronger. Thus CCl₄ is more volatile.

5 0
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