PV-nRT 9. Given the equation above, called the Ideal Gas Law, determine how many

Question

PV-nRT 9. Given the equation above, called the Ideal Gas Law, determine how many moles of gas were in the syringe that you used, if the volume was 11.5 mL at room temperature (23 °C). Remember to make your units cancel as you solve. 0.88268-0.0821(1296.15)n 0.88286/24.31392 0.03631n The gas in your syringe and the copper tubing was air, a mixture of gases. Calculate the density 23 °C. The average molecular mass of dry air is 28.97 g/mole. 23+273 296 ? 1 atm (28.97 28.97 296 K (00821 .1.19 g/L 10. of air in your syringe (we'll assume it was dry for this calculation) in g/L at 2897 28.97 1,19 g/L

Explanation / Answer

They have multiplied volume ( 0.0115L) with standard atmospheric pressure 76cmHg. However this is wrong because the universal gas constant R's value is 0.0821 and the unit for pressure should be atm. The correct method should be:

1atm* 0.0115L= 0.0821*296.15K*n

n= 0.00047moles

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