Is the ratio of the partial pressures of the two gases at 90°C equal to the ratio of their volumes under standard conditions?
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At 90°C, gases A and B flow inside a container. The partial pressure of A is 80 kPa, while that of B is 30 kPa. It is also known that the flow rate of B is 250 Nm3/h. What is the flow rate of A? Which of the following two calculation methods (1) and (2) is correct? If neither is correct, please provide the correct method. Thank you.Method (1): The volumetric flow rate of A = 250 × 80/30 = 667 Nm3/h.
Method (2): First, convert the volume of B at 90°C. Using the equation P1V1/T1 = P2V2/T2, we get 101325 × 250/273.15 = 30000 × V2/(273.15 + 90). Thus, the volume of gas B at 90°C is V2 = 1123 m3. The volume of gas A at 90°C is then 1123 × 80/30 = 2994 m3. Next, convert this volume of A to standard conditions: 80000 × 2994/(273.15 + 90) = 101325 × V/273.15. Therefore, the volumetric flow rate of A is 1778 Nm3/h
The standard state generally refers to 20 degrees, not 273.15K