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Vsevolod [243]
2 years ago
8

A sample of CO2 gas at 100 degrees Celsius has a volume of 250 mL at 760 mm Hg. How many moles of CO2 are present

Chemistry
1 answer:
Fed [463]2 years ago
6 0

There are 8.16 × 10-³ moles of CO2 gas at 100°C with a volume of 250 mL at 760 mm Hg.

HOW TO CALCULATE NUMBER OF MOLES:

The number of moles of a sample of gas can be calculated using the following formula:

PV = nRT

Where;

  • P = pressure of gas (atm)
  • V = volume (L)
  • n = number of moles (mol)
  • R = gas law constant (0.0821 Latm/molK)
  • T = temperature (K)

According to this question;

  • P = 760mmHg = 1 atm
  • T = 100°C = 100 + 273 = 373K
  • V = 250mL = 0.250L
  • n = ?

1 × 0.250 = n × 0.0821 × 373

0.250 = 30.62n

n = 0.250 ÷ 30.62

n = 8.16 × 10-³mol

Therefore, there are 8.16 × 10-³ moles of CO2 gas at 100°C with a volume of 250 mL at 760 mm Hg.

Learn more about number of moles at: brainly.com/question/4147359

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Read 2 more answers
How do you do this? very confused
Vlad [161]
The problem you have written you almost have it solved.  Take the moles that you have calculated and multiply that by the molecular weight to get the grams.

The STP problem:
use the moles you calculated along with 1 atm for Pressure, and 273 for the temperature and plug into the PV = nRT equation.  (also use 0.0821 for R)

From there you can solve for the volume

Hope this helps!
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