A) What volume is occupied by 2.24 grams of nitrogen gas at a pressure of 1450 t

Question

A) What volume is occupied by 2.24 grams of nitrogen gas at a pressure of 1450 torr and a temperature of -10 °C?

B) A balloon is inflated to a volume of 3.34 L at sea level, where the pressure is 1.00 atm and the temperature is 18 °C. Suppose the balloon is released and rises to a point where the pressure is 575 torr. What is the temperature if the new volume of the balloon is 3.00 L at a pressure of 575 torr?

C)What is the volume of 0.00325 moles of oxygen gas at STP?

D)Draw the Lewis structure for XeCl4 & indicate the number of valence electrons

-what is the molecular geometry for XeCl4?

Explanation / Answer

A) V = nRT/P = (2.24/28)*0.0821*263.15/1.91 = 0.9 L

B) P1V1/T1 = P2V2/T2

3.34*760/291.15 = 575*3/T2

T2 = 197.85 K = 75.3 c

C) At STP 1 mol occupies 22.4 L

   so that,

Volume of O2 = 0.00325*22.4 = 0.0728 L

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