Question

1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL...

1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL at 25 oC gravity = 9.8 m/s2
R = 0.082 L.atm/mol.K    PV = nRT            Force = mass x acceleration
Pressure = Force/area

Today’s atmospheric pressure is 32.0” of mercury. What is the pressure in ‘atm’ units?

The burette used in the lab has a cross-section area of 1 cm2 so that a height of 1 cm provides a volume of 1 cm3 (that is 1 mL).
(a) What is the mass of mercury in a burette filled up to a height of 76 cm? Give the answer in kg units.
(b) What is the force of this 76 cm mercury column acting downward due to gravity? [Note: As long as you use SI units for mass and acceleration, the SI unit for force is Newtons]
(c) Pressure is Force per unit area. What is pressure due to this 76 cm mercury column? [Note: the cross sectional area of the column is given in non SI unit. As long force and area are in SI units, the SI unit for pressure is Pascal.]
(d) You have learned that 1 atm pressure is 76 cm of mercury. Based on the math you did in this problem, what is the value of 1 atm in Pascal units?

(a) Container A has a volume of 5.0 L and is filled with 5.0 grams of hydrogen gas at 25oC. What will be the pressure of hydrogen gas in the container?
(b) Another container (container B) has a volume of 10.0 L and is also filled with 5.0 grams of hydrogen gas at 25 oC. What will be the pressure of hydrogen gas in this container?
(c) If container A and container B are connected with each other using a small glass tube to allow free flow of gas between them, what will happen to the pressure of hydrogen gas? If it is affected, find the new value.

N2 (g) + 3 H2 (g) à 2 NH3 (g). In a reaction, 24.0 g of nitrogen and 14.0 g of hydrogen are reacted to produce ammonia in 5.0 L rigid container at 25 oC .
(a) What will be the pressure inside the container before the reaction starts?
(b) What is the limiting reactant in this reaction?
(c) After the reaction is completed, how many moles of product and how many moles of unreacted reactant will be present?
(d) What will be the pressure in the container after the reaction is complete?

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