1. A small piece of zinc reacts with dilute HCl to form H2, which is collected over water at 16°C into a large flask. The total pressure is adjusted to barometric pressure (752 torr), and the volume is 1538 mL. Use Table 5.2 to help calculate the partial pressure and mass of H2.

Question

1. A small piece of zinc reacts with dilute HCl to form H2, which is collected over water at 16°C into a large flask. The total pressure is adjusted to barometric pressure (752 torr), and the volume is 1538 mL. Use Table 5.2 to help calculate the partial pressure and mass of H2.
__torr
__g

DrBob222 · Accepted Answer

I don't have Table 5.2 but I assume that is vapor pressure of water.
Total pressure (752 torr) = Partial pressure H2 + partial pressure of H2O.
Look in the table at 16 C and pick up the vapor pressure of water (partial pressure of water), subtract that from 752 to find the partial pressure hydrogen.

Carter · Answer

So, how do I get the grams ? Thank you.

DrBob222 · Answer

Again, I don't know what is in Table 5.2. Perhaps it will help. If it isn't in Table 5.2, then try using PV = nRT. You know P, V, R, and T, Calculate n = number of moles. Then mols dry gas x molar mas = grams.

Carter · Answer

I got it. Thank you so much.