= 115mmHg Constants| Periodic Table You may want to reference (Pages 276 -279) S

Question

= 115mmHg Constants| Periodic Table You may want to reference (Pages 276 -279) Section 8.7 while completing this problem Correct A mixture of nitrogen (N2) and helium has a volume of 290 mL at 36 C and a total pressure of 757 mmHg According to Dalton's law, the total pressure of this gas mixture is the sum of the partial pressure of helium and the partial pressure of nitrogen. Given that the total pressure is 757 mmHg, the partial pressure of nitrogen can be determined by subtracting the partial pressure of helium from the total pressure partial pressure of nitrogen gas = 757 mmHg-42 mmHg = 715 mmHg Part B What is the final volume, in liters, of the nitrogen at STP? Express your answer to two significant figures and include the appropriate units Vhinal-ValueUnits Submit X Incorrect; Try Again; 6 attempts remaining

Explanation / Answer

part B)

pressure of N2 = 715 mmHg = 0.941 atm (P1)

volume = 290 mL = 0.290 L (V1)

temperature = T1 = 36 oC = 309.15 K

pressure = P2 = 1 atm

temperature = 273 K

P1 V1 / T1 = P2 V2 / T2

0.941 x 0.290 / 309.15 = 1 x V2 / 273

V2 = 0.241 L

volume of N2 = 2.4 x 10^2 mL

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