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3 years ago

Which of the following would remain a liquid longer as temperature continues to drop?

Chemistry

2 answers:

Len [333]3 years ago

8 0

Answer:

Octane

Explanation:

Hydrocarbons are composed of carbon and hydrogen atoms and are generally non-polar. The only intermolecular force of attraction between hydrocarbons is the weak van der waals interaction. Longer the hydrocarbon chain, stronger will be this interaction.

In the given options:

Propane = C3H8

Octane = C8H18

Hexane = C6H14

Ethane = C2H6

Thus, octane is has the longest chain and will have the strongest van der waal interaction which will allow the molecule to stay in a liquid state longer.

viktelen [127]3 years ago

3 0

I just took a test with this question and got the answer wrong for saying ethane. The correct answer is propane.

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At 47c a gas has a pressure of 140kpa. The gas is cooled until the pressure decreases to 105kpa. If the volume remains constant,

IgorC [24]

Answer:

The final temperature is equal to 240 K or -33.15°C

Explanation:

Given that,

Initial temperature of the gas, T₁ = 47°C = 320 K

Initial pressure, P₁ = 140 kpa

Final pressure, P₂ = 105 kpa

We need to find the final temperature if the volume remains constant. The relation between temperature and pressure is given by :

$P\propto T$

$\dfrac{P_1}{P_2}=\dfrac{T_1}{T_2}\\\\T_2=\dfrac{P_2T_1}{P_1}\\\\T_2=\dfrac{105\times 320}{140}\\\\T_2=240\ K\\\\T_2=-33.15^{\circ} C$

So, the final temperature is equal to 240 K or -33.15°C.

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3 years ago

As a liquid is added to a beaker, the pressure exerted by the liquid on the bottom of the beaker does what

ololo11 [35]

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2 years ago

22.4l of ammonia is reaxts with 1.406 mole of oxygen to produce NO and h2o .1.what volume of no is produced at ntp

IceJOKER [234]

Answer:

The volume of NO is 22.4L at STP

Explanation:

Based on the reaction:

2NH3 + 5/2O2 → 2NO + 3H2O

2 moles of NH3 react with 5/2 moles of O2 to produce 2 moles of NO.

To solve this question, we need to find the moles of each reactant in order to find the limiting reactant as follows:

Moles NH3 -Molar mass: -17.01g/mol-

Using PV = nRT

PV/RT = n

Where P is pressure = 1atm at STP

V is volume = 22.4L

R is gas constant = 0.082atmL/molK

T is absolute temperature = 273.15K

1atm*22.4L/0.082atmL/molK*273.15K = n

n = 1.00 moles of NH3

For a complete reaction of 1.00 moles of NH3 are needed:

1.00 moles NH3 * (5/2moles O2 / 2moles NH3) = 1.25 moles of O2

As there are 1.406 moles of O2, the limiting reactant is NH3

The moles of NO produced are the same than moles of NH3 because 2 moles of NH3 produce 2 moles of NO. The moles of NO are 1.00 moles

And as 1.00moles of gas are 22.4L at STP:

<h3>The volume of NO is 22.4L at STP</h3>

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