In need of help setting up each of these problems.

Under the conditions in a laboratory experiment, 0.0513 grams of aluminum (At. Wt.=27.0) was reacted with excess hydrochloric acid to produce hydrogen gas according to the following balanced equation:
2 Al+ 6 HCL -> 2 AlCl3+ 3 H2

A) Determine the number of moles of H2 evolved from the quantity of aluminum when collected over water.

B) If the Volume of gas generated was 75.0 mL and the temperature was 27.0 degrees celsius, determine the total pressure of the hydrogen gas evolved from the quantity of aluminum stated above.

C) The vapor pressure of water at 27.0 degrees celsius was 26.7 mmHg, determine the partial pressure of the hydrogen gas collected in mmHg.

A.

mols Al = grams/atomic mass = ? This is n in part B.

B.
Use PV = nRT. You know n, R, V and T. Remember V is in L, T in kelvin, R=0.08205. Solve for P in atm.

C.
Ptotal = pH2 + pH2O. Ptotal and pH2O are given. Solve for pH2.

To set up each of these problems, we need to use the given information and apply the appropriate formulas or equations. Let's break down each problem and go through the setup step by step:

A) Determine the number of moles of H2 evolved from the quantity of aluminum when collected over water.

To determine the number of moles of H2, we need to use the balanced equation and the molar ratio between aluminum (Al) and hydrogen gas (H2).

Given:
Mass of aluminum, m = 0.0513 grams
Atomic weight of aluminum, At. Wt. (Al) = 27.0 g/mol

Step 1: Convert the mass of aluminum (in grams) to moles.
Number of moles of Al = Mass of Al / Atomic weight of Al

Step 2: Use the balanced equation to find the moles of H2.
From the balanced equation, we know that 2 moles of Al react to produce 3 moles of H2.
Therefore, the molar ratio of Al to H2 is 2:3.

Moles of H2 = Moles of Al * (3 moles of H2 / 2 moles of Al)

Now you have the number of moles of H2 evolved from the given quantity of aluminum.

B) If the Volume of gas generated was 75.0 mL and the temperature was 27.0 degrees Celsius, determine the total pressure of the hydrogen gas evolved from the quantity of aluminum stated above.

To determine the total pressure of the hydrogen gas, we need to use the ideal gas law equation:

PV = nRT

Given:
Volume of gas, V = 75.0 mL = 0.075 L
Temperature, T = 27.0 degrees Celsius = 27.0 + 273.15 Kelvin (convert to Kelvin)

Step 1: Convert temperature to Kelvin.

Now use the ideal gas law equation to solve for pressure (P):
P = nRT / V

Substitute the known values to find the total pressure of the hydrogen gas evolved.

C) The vapor pressure of water at 27.0 degrees Celsius was 26.7 mmHg. Determine the partial pressure of the hydrogen gas collected in mmHg.

The partial pressure of the hydrogen gas collected can be calculated by subtracting the vapor pressure of water from the total pressure obtained in part B.

Partial pressure of H2 = Total pressure - Vapor pressure of water

Substitute the known values to find the partial pressure of the hydrogen gas collected.