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JulsSmile [24]
4 years ago
14

An element can be identified as either a ________, __________, or a __________

Chemistry
2 answers:
motikmotik4 years ago
5 0
Liquid or a solid :)

dexar [7]4 years ago
4 0
Solid, Liquid, or a Gas
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How many moles are in a sample of Sodium that contains 1.806 x 1024 atoms?
Ad libitum [116K]

Answer: 3 moles Na

Explanation: To find the number of moles of Na, divide the number of atoms of Na with the Avogadro's Number.

1.806x10²⁴ atoms Na x 1 mole Na / 6.022x10²³ atoms Na

= 2.99 or 3 moles Na

3 0
4 years ago
You are investigating an organic compound. You discover that it is an aromatic compound often used as flavoring. What type of co
Dafna1 [17]
Aldehyde is the answer for Plato users!
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4 years ago
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A solution of methanol and water has a mole fraction of water of 0.312 and a total vapor pressure of 21 torr at 39.9 degrees C.
Elan Coil [88]

Answer:

Explanation:

Given the details, we can say that

Pure methanol is a volatile solvent as the vapour pressure has a high value. This means that methanol - methanol intermolecular forces are weak in comparisson to water - water forces. When having about 30% of water in a methanol mixture, the mixture Pv decreased, showing that it is not a volatile mixture, so then there are strong intermolecular interactions between methanol - water, part of it due to the hydrogen bonds.

8 0
3 years ago
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A 1.00 L flask is filled with 1.15 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pres
tatiyna

Answer:

The partial pressure of argon in the flask = 71.326 K pa

Explanation:

Volume off the flask = 0.001 m^{3}

Mass of the gas = 1.15 gm = 0.00115 kg

Temperature = 25 ° c = 298 K

Gas constant for Argon R = 208.13 \frac{J}{kg k}

From ideal gas equation P V = m RT

⇒ P = \frac{m R T}{V}

Put all the values in above formula we get

⇒ P = \frac{0.00115}{0.001} × 208.13 × 298

⇒ P = 71.326 K pa

Therefore, the partial pressure of argon in the flask = 71.326 K pa

4 0
4 years ago
Methane at 10 mpa and 300 k is heated at constant pressure until its volume has increased by 80 percent. determine the final tem
katovenus [111]
When you assume that the gas is behaving ideally, the gas molecules are very far from each other that they do not have any intermolecular forces. If it behaves this way, you can assume the ideal gas equation:

PV = nRT, where

P is the pressure
V is the volume
n is the number of moles
R is a gas constant
T is the absolute temperature

When the process goes under constant pressure (and assuming same number of moles),

P/nR = T/V = constant, therefore,

T₁/V₁=T₂/V₂

If V₂ = V₁(1+0.8) = 1.8V₁, then,

T₂/T₁ = 1.8V₁/V₁

Cancelling V₁,

T₂/300=1.8
T₂ =540 K

If you do not assume ideal gas, you use the compressibility factor, z. The gas equation would now become

PV =znRT

However, we cannot solve this because we don't know the value of z₁ and z₂. There will be more unknowns than given so we won't be able to solve the problem. But definitely, the compressibility factor method is more accurate because it does not assume ideality.

7 0
3 years ago
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