A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas (n1), and its volume is 42.0 L (V1). If 0.500 mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?

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A) A cylinder, with a piston pressing down with a constant pressure, is filled with 2.20 moles of a gas (n1), and its volume is 42.0 L (V1). If 0.300 mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?

B)Imagine that you have an ideal gas in a 9.00 L container, and that 2150 molecules of this gas collide with a square-inch area of the container at any given instant.

If the volume is increased to 36.0 L at constant temperature, how many collisions will occur per square inch of this larger container?

C) What volume of O2 at 798 mmHg and 37 âC is required to synthesize 14.5 mol of NO?

The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO)gas as shown by the unbalanced equation given here:

?NH3(g)+?O2(g)â?NO(g)+?H2O(g)NH3(g)+?O2(g)â?NO(g)+?H2O(g)

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A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas (n1), and its volume is 42.0 L (V1). If 0.500 mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?

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