A rigid container holds 3.20 moles of an ideal gas at an absolute pressure of 1.

Question

A rigid container holds 3.20 moles of an ideal gas at an absolute pressure of 1.92 Times 10^5 Pa and a temperature of 40.0 degree C. What is the volume of the rigid container? The container will explode at a pressure of 2.48 Times 10^5 Pa. What maximum gas temperature (in Celsius) docs this correspond to? The water behind a dam built across one end of a very large lake is 25.2 m deep. A small hole, 1.00 cm in diameter, opens 1.40 m above the lakebed. A small Dutch boy realizes his finger fits in the hole, allowing him to plug the leak and stop the water from flowing. What is the absolute pressure on his finger? What force does the pressure of the water at the hole exert on his 1.00-cm-diameter finger?

Explanation / Answer

The ideal gas law states that

PV = nRT

In this equation, 'P' is the pressure in atmospheres, 'V' is the volume in liters, 'n' is the number of particles in moles, 'T' is the temperature in Kelvin and 'R' is the ideal gas constant (0.0821 liter atmospheres per moles Kelvin)

P = 1.92*105 Pa = 1.894*10-5 atm

So V = nRT/P = 3.20*0.081*(273+40)/(1.894*10-5) = 42.855*105 litre

b) New Preasure = 2.48*105 Pa = 2.447*10-5 atm

So, P'V = nRT'

T' = 0.2592 K = -272.8908 0C

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