If 0.1453 g of aluminum metal reacted with excess hcl(aq) in an experiment conducted in denver, co, calculate the theoretical volume of h2 that would be collected over water if the temperature of was 17.0 c and the atmospheric pressure was 29.25 inches of hg. (use textbook r value)

0,1966L

Explanation:

The reaction of aluminium with HCl is:

Al(s) + 3HCl(aq) → AlCl₃ + ³/₂H₂(g)

Moles of aluminium that react are:

0,1453g×= 5,385x10⁻³ moles of Al

As 1 mole of Al produce ³/₂ moles of H₂(g), the moles of H₂ are:

5,385x10⁻³ moles of Al× = 8,078x10⁻³ mol H₂(g)

To find the volume H₂ occupies you need to use:

Where n are moles (8,078x10⁻³ mol H₂(g))

R is gas constant (0,082atmL/molK)

T is temperature (17,0°C+273,15 = 290,15K)

And P is pressure (29,25 inches of Hg/29,921= 0,9776 atm)

Replacing:

I hope it helps!

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

that's what i got you can count the number of atoms