Question

A balloon contains 5L of oxygen at a pressure of 90 kPa. How much oxygen will the ballon contain if the pressure is lowered to 67 kPa.

Answer 1

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Answer 2

We have that all (ideal) gases obey the fundamental gas equation: PV=nRT where P is the Pressure, V is the Volume, n is the number of moles, R is a universal constant and T is the temperature in Kelvin. In this process, we have that both the number of moles and the temperature stays the same. So if we denote by i the initial conditions and by f the final conditions of the gas, we have:$P_{i} * V_{i}=nRT= P{f}*V{f}$ . Hence, if we solve for the final Volume we get: $V_{f} = \frac {V_{i}*P_{i} }{P_{f}}$ . Now we know all the other variables; substituting we get that the final volume is 6.7 L (6.716 L ).