When Zn reacts with HCl solution, the products are H2 gas and ZnCl2. A volume of 426 mL of H2 gas is collected over water at a total pressure of 751 mmHg and 16âC. The vapor pressure of water at 16âC is 14 mmHg.
Zn(s)+HCl(aq) â H2(g)+ZnCl2(aq).

1.What was the partial pressure of the H2 gas?

2.How many moles of H2 gas were produced in the reaction?

answer

watching

940

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Trinidad TremblayLv2

13 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Zinc reacts with aqueous sulfuric acid to form hydrogen gas:

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

In an experiment, 201 mL of wet H₂ is collected over water at 27 Â°C and a barometric pressure of 732.78 torr. The vapor pressure of water at 27 Â°C is 26.74 torr. The partial pressure of hydrogen in this experiment is __________ atm.

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 Â°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 Â°C.

2) Sodium metal reacts with water to produce hydrogen gas according to the following equation:

2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)

The product gas, H2, is collected over water at a temperature of 20 Â°C and a pressure of 746 mm Hg. If the wet H2 gas formed occupies a volume of 6.33 L, the number of grams of H2 formed is g. The vapor pressure of water is 17.5mm Hg at 20 Â°C.

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.)