How many grams of hydrogen gas would be produced from the use of 9.5 miles of aluminum?

28.5g of H2

Explanation:

First, let us write a balanced equation for the reaction. This is illustrated below:

2Al + 6HCl —> 2AlCl3 + 3H2

From the balanced equation,

2moles of Al produced 3moles of H2.

Therefore, 9.5 moles of Al will produce = (9.5x3)/2 = 14.25moles of H2.

Now let us convert 14.25moles of H2 to grams as illustrated below:

Molar Mass of H2 = 2x1 = 2g/mol

Number of mole H2 = 14.25moles

Mass of H2 =?

Number of mole = Mass /Molar Mass

Mass = number of mole x molar Mass

Mass of H2 = 14.25 x 2

Mass of H2 = 28.5g

first let us lay out the formula for potential

and kinetic energy:

pe = mgh

ke = (mv^2)/2

where: m=mass, v=velocity, g=gravitational

acceleration, h=height

calculating for mass using the known values of

pe:

340j = m (9.81 m/s^2) (50ft) (1m/3.28ft)

m = 2.27 kg

the law of conservation of energy states that

energy is neither created nor destroyed. therefore, the change in kinetic

energy from 50 ft to 35 ft would be equal to the change in potential energy

from 50 ft to 35 ft. however it would be opposite in signs since one is losing

while other is gaining.

ke(35ft) – ke(50ft) = - [ pe(35ft) – pe(50ft]

ke(50ft) = 0 since the brick is initially at rest

ke(35ft) = 340j - 2.27kg (9.81 m/s^2) (35ft)

(1m/3.28 ft)

ke(35ft)

= 102.38 j