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vivado [14]
3 years ago
9

How many moles of ammonia gas occupy 50 mL at at 700 kPa and 30.0 0C?

Chemistry
1 answer:
nalin [4]3 years ago
6 0

For the conversions

I will start with pressure
1atm=101.3kPa
x =700kPa
x=700kPa/101.3kPa
x=6.91atm

Temperature
273K+30.00C
303K

Volume
1L=1000ml
x =50ml
x=0.05L

PV=nRT
6.91*0.05=n*0.08206*303
0.3455=24.86418n
0.3455/24.86418=n
0.0138=n
number of moles = 0.0138moles

Note: 0.08206 is the gas constant in this case
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Answer:

B

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If 725 ml of N² gas is at 1 atm, what volume will it have at 1.4 atm?​
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Answer:

518 mL

Explanation:

We can solve this using Boyle's Law Formula

P1V1 = P2V2

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here , the initial pressure is 1 atm and the initial volume is 725mL

we are given the final pressure 1.4 and we need to find the final volume

so we have p1v1 = p2v2

==> plug in p1 = 1 , v1 = 725 mL and p2 = 1.4

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2 years ago
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How are intermolecular forces of attraction, vapor pressure, and boiling point related?
monitta

Answer:

Intermolecular forces (IMFs) can be used to predict relative boiling points. The stronger the IMFs, the lower the vapor pressure of the substance and the higher the boiling point. Therefore, we can compare the relative strengths of the IMFs of the compounds to predict their relative boiling points.

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200/3 M which is approximately equal to 66.6667 M

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Substitute with the givens in the above equation to get the molarity as follows:
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