A cylinder with a capacity of 10 cubic meters contains hydrogen under a pressure of 2.03 MPa.

A cylinder with a capacity of 10 cubic meters contains hydrogen under a pressure of 2.03 MPa. How much volume is needed to store the same amount of hydrogen at normal atmospheric pressure and the same temperature?

To find the required volume of the vessel for storing the taken hydrogen, we use the proportion (we take into account that the taken hydrogen has a constant temperature): P1 * V1 = Pн.у. * V2, whence we express: V2 = P1 * V1 / Pн.у.

Constants and variables: P1 – initial pressure of taken hydrogen (P1 = 2.03 MPa = 2.03 * 10 ^ 6 Pa); V1 is the capacity of the first cylinder (V1 = 10 m3); Pn.y. (normal atmospheric pressure) = 101325 Pa.

Let’s make a calculation: V2 = P1 * V1 / Pн.у. = 2.03 * 10 ^ 6 * 10/101325 = 200.3 m3.

Answer: After reducing the pressure, a cylinder with a capacity of 200.3 m3 is required to store the taken hydrogen.



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