Question

Hydrogen gas is produced when zinc reacts with sulfuric
acid:

Zn(*s*)+H2SO4(*a**q*)→ZnSO4(*a**q*)+H2(*g*)

If 155 mL of wet H2 is collected over water at 24 ∘C and a barometric pressure of 736 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)

Answer #1

1st find the moles of H2 produced

we have:

P = 736 torr - 22.38 torr

= 713.62 torr

= (713.62/760) atm

= 0.939 atm

V = 155.0 mL

= (155.0/1000) L

= 0.155 L

T = 24.0 oC

= (24.0+273) K

= 297 K

find number of moles using:

P * V = n*R*T

0.939 atm * 0.155 L = n * 0.08205 atm.L/mol.K * 297 K

n = 5.972*10^-3 mol

from reaction,

moles of Zn reacted = moles of H2 produced

= 5.972*10^-3 mol

Molar mass of Zn = 65.38 g/mol

we have below equation to be used:

mass of Zn,

m = number of mol * molar mass

= 5.972*10^-3 mol * 65.38 g/mol

= 0.3904 g

Answer: 0.390 g

Zinc reacts with aqueous sulfuric acid to form hydrogen gas:
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) In an experiment, 225 mL of
wet H2 is collected over water at 27 °C and a barometric pressure
of 765torr. How many grams of Zn have been consumed? The vapor
pressure of water at 27 °C is 26.74 torr.

Zinc metal reacts with hydrochloric acid according to the
following balanced equation.
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
the hydrogen gas is collected over water at a temperature of
20.0 degrees celsius and a total pressure of 775.2 mmHg. a total of
1.85 L of gas is collected. the vapor pressure of water at 20.0
degrees celsius is 17.55 mmHg. what is the mass of hydrogen gas (in
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The hydrogen gas from the reaction: Zn(s)
+2HCl(aq)->ZnCl2(aq)+H2(g) is bubbled through water for
collection. 250mL of Hydrogen gas is collected at 25o Celsius. The
total pressure is 1.032 atm. Calculate the partial pressure of the
hydrogen gas and the mass of Zinc required to produce that gas.
(The vapor pressure of water is 23.76 torr at 25oCelsius).

A)
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
757 mm Hg. If the wet
H2 gas formed occupies a volume of
7.17L, the number of moles of Zn
reacted was ___________ mol. The vapor pressure of water is
17.5 mm Hg at 20 °C.
B) Oxygen...

Small amounts of hydrogen gas are often produced by reaction of
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temperature is 17.54 mm Hg.) will be produced by the reaction of
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A 0.442 gram sample of a metal, M, reacts completely with
sulfuric acid according to:
M(s) + H2SO4(aq) -->
MSO4(aq) + H2(g)
A volume of 201 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

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sulfuric acid according to: M(s) + H2SO4(aq) ----> MSO4(aq)
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water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

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sulfuric acid according to:
M(s) + H2SO4(aq) → MSO4(aq) + H2(g)
A volume of 205 mL of hydrogen is collected over water; the
water level in the collecting vessel is the same as the outside
level. Atmospheric pressure is 756.0 Torr and the temperature is 25
°C. The vapor pressure of water at various temperatures can be
found in this table. Calculate the molar mass of the metal.

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(Water vapor pressure at 34°C = 39.90 mmHg)
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