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A 290 ml gas sample contains argon and nitrogen at a temperature of 65 ?c. the total pressure of the sample is 725 mmhg and the partial pressure of argon is 231 mmhg. what mass of nitrogen is present

Respuesta :

BlueSky06
The partial pressure of nitrogen in the problem is 725 - 231 = 494 mmHg. 
494 / 760 = 0.650 atm. To continue, we will use the ideal gas equation to find the mole of N2 and from that, we can find the mass of N2.

PV = nRT ----> n= PV/RT

Find the mole of Nitrogen
Given P=0.650 atm

n= (0.650)x(255/1000) / (0.082 x 338)
  = (0.650) (0.255) / 27.716
  =  0.16575 / 27.716
  = 0.0060 moles 

Find the mass of nitrogen 
G= n x Mr (N2)
   = 0.0060 x 28
   = 0.168 grams 

So the mass of nitrogen is 0.168 
okpalawalter8

The mass of nitrogen is mathematically given as

Ng= 0.168 grams

What mass of nitrogen is present?

Generally, the equation for the ideal gas  is mathematically given as

PV = nRT

Therefore

n= PV/RT

Hence

n= (0.650)x(255/1000) / (0.082 x 338)  

n (0.650) (0.255) / 27.716  

n= 0.0060 moles  

Therefore the mass of nitrogen  is

Ng= n x Mr (N2)

Ng = 0.0060 x 28

Ng= 0.168 grams

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