When the experiment was carried out, the temperature was 22 oC and atmospheric pressure was 1.007 atm. Using the Ideal Gas Law and the measured volume of H2 gas collected to find the number of moles of H2 gas produced in the experiment.

number of moles of =4.16mol

Explanation:

experiment data:

temperature= =273+22 k=295k

pressure=1.007 atm

volume is missing so assuming volume-=100L

using ideal law relationship

ideal gas means gas which occupies negligible space and there is no interaction between the molecules of gases.

PV=nRT

put all the experimental data, we get

n=4.15 mol

number of moles of =4.16mol

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.

hypostyle hall;