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Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g) Typically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 240. mL of hydrogen gas is collected at 30.∘C and has a total pressure of 1.032 atm by this process. What is the partial pressure of hydrogen gas in the sample? How many grams of zinc must have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at 30∘C.)

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Lulama Klaas
Lulama KlaasLv10
28 Oct 2020

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Related questions

Small quantities of hydrogen gas can be prepared in the lab by addition of hydrochloric acid to zinc. The gas is typically collected over water (what does collected over water mean?). What volume of hydrogen can be collected from 0.625g Zn? The total pressure is 784torr at 30oC. Water has a vapor pressure of 32torr at 30oC.

Zn(s) + 2 HCl(aq) --> ZnCl2(aq) + H2)g)

a) 30mL b) 157mL c) 240mL d) 316mL e) 564mL

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Zn (s) + H2SO4 (aq) → H2 (g) + ZnCl2 (aq)

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1) Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation:

Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)

The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 750 mm Hg. If the wet H2 gas formed occupies a volume of 9.18 L, the number of grams of H2 formed is g. The vapor pressure of water is 17.5mm Hg at 20 °C.

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