Analysis of aluminum-zinc alloy

Mass of gelatin capsule 0.1284 g ambient temp. 22c
mass of capsule plus alloy sample 0.3432g ambient temp_________K
mass of alloy sample, m__________g barometric pressure 745 mm Hg
mass of empty beaker 144.5g Vapor pressure at
H2O at t_____________mm Hg
mass of beaker plus displaced
water 368.9
mass of displaced water ___________g Pressure of dry H2,
ph2 ________________mm Hg
volume of displaced water
(density = 1.00 g/ml)_____________ml Pressure of dry _________atm
volume, v, of h2 = volume of displaced water __________ml_________liters

find the number of moles of h2 evolved nh2(v in liters, ph2 in atm, T in K, R= 0.0821 liter-atm/mole K) _____________________moles H2

find Nh2 the number of moles of H2 per gram of sample_________moles H2/g

find the % Al in the sample from the graph prepared _____________% Al

find the % Al in sample ____________________% Al

(please if you could help me filling these blanks)

It looks like this is a practical/experiment type questions that you should already have your the results. It would be easier if you enter your values for the temperatures and pressures and leave the mole calculations and % for help.

To find the values for the blanks in the given question, we will go step by step:

1. Ambient temperature:
The given ambient temperature is 22°C. To convert this to Kelvin, you need to add 273 to the Celsius temperature:
22°C + 273 = 295 K (fill in the blank with 295 K).

2. Mass of alloy sample, m:
The mass of the capsule plus alloy sample is given as 0.3432 g, and the mass of the gelatin capsule is given as 0.1284 g. Therefore, the mass of the alloy sample can be obtained by subtracting the mass of the capsule from the mass of the capsule plus alloy sample:
0.3432 g - 0.1284 g = 0.2148 g (fill in the blank with 0.2148 g).

3. Vapor pressure of H2O at t:
The vapor pressure of water at a specific temperature, denoted as "t," is missing. You need to consult a vapor pressure table or use a reliable source to find the vapor pressure of water at the given ambient temperature of 22°C.

4. Pressure of dry H2, ph2:
The pressure of dry H2 is missing. The pressure of dry H2 can be measured using a gas pressure sensor or obtained from a reliable source.

5. Volume of displaced water:
The volume of displaced water is given as 368.9 g. Since the density of water is 1.00 g/mL, the volume can be obtained by dividing the mass of the displaced water by the density:
368.9 g / 1.00 g/mL = 368.9 mL (fill in the blank with 368.9 mL).

6. Volume, v, of H2:
The volume, v, of H2 is equal to the volume of displaced water. Therefore, fill in the blank with 368.9 mL.

Now let's move on to the calculations:

1. Number of moles of H2 evolved, nH2:
To find the number of moles of H2 evolved, you need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure of gas (in atm)
V = volume of gas (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 liter-atm/mole K)
T = temperature in Kelvin (from the given ambient temperature in Kelvin)

Fill in the blank with the given values:
nH2 = (ph2 * v) / (R * T)

2. Number of moles of H2 per gram of sample, Nh2:
To find the number of moles of H2 per gram of sample, divide the number of moles of H2 by the mass of the alloy sample:
Nh2 = nH2 / m

3. % Al in the sample from the prepared graph:
The % Al in the sample can be obtained from a graph or other data provided separately. Fill in the blank with the value obtained from the graph or data.

4. % Al in the sample:
The % Al in the sample is missing. This value can be obtained from experimental data or calculations based on the composition and properties of the aluminum-zinc alloy.