Question

Hydrogen gas is generated when acids come into contact with certain metals. When excess hydrochloric acid reacts with 2.2 g of (the metal product is ), what volume of hydrogen gas is collected at a pressure of 0.98 atm and a temperature of 20.°C?

Answer 1

To solve the problem it is necessary to apply the concepts related to Byle's Law and Avogadro's Law.

The ideal gas equation would help us find the final solution to the problem, defined by

$PV = nRT$

Where,

T= Temperature of the gas

R = Universal as constant

n = number of moles

V = Volume

P = Pressure

For our case we have that the mass of Zn is 2.2g in moles would be

$[tex]Zn = \frac{2.2}{65}$[/tex]

$Zn = 0.0338$

We know that 1 mole of hydrogen gas is proceed by 1 mole of zinc and the result is $Zn^{2+}$, then Hydrogen can produce the same quantity,

$H_2 = 0.0338$

Applying the previous equation we have that

$V= \frac{nRT}{P}$

$V = \frac{0.0338*0.08206*293.15}{0.98}$

$V = 0.829L$

Therefore the volume of hydrogen gas is collected is 0.829L