Answer to Question #270439 in General Chemistry for gimar

Question

Calculate the pressure of hydrogen gas produced if 50 grams of Aluminum

reacts with 250 grams of Hydrochloric acid. The Hydrogen gas is collected

at 2.75 L vessel at 80.6 ℉.

Answer 1

Al +6HCl $\to$ 2AlCl₃ + 3H₂

50g 250g

P= nRT / V

Moles of All

=m / RFM

= 50/27

= 1.8519moles

Moles of HCl= m/ RFM

= 250 / 36.5

= 6.8493 moles

Moles of Al = 6.8493 / 6

= 1.1416moles

Moles of H₂ =

( 3 × 6.8493 / 6 ) moles

n = 3.42465 moles

V= 2.75l

T=86.6 °F

If 32°F= 0 °C

$\therefore$ 80.6 ° F

80.6 / 32 × 1

= 2.5188 ° C

T in $\kappa$

2.51888 + 273.15

=275.6688k

r = nRT / V

(3.42465 × 8.3142 × 275.

6688k ) / 2.75

= 2854.2472 atm