1. A small piece of zinc reacts with dilute HCl to form H2, which is collected over water at 16°C into a large flask. The total pressure is adjusted to barometric pressure (752 torr), and the volume is 1538 mL. Use Table 5.2 to help calculate the partial pressure and mass of H2.

__torr
__g

I don't have Table 5.2 but I assume that is vapor pressure of water.

Total pressure (752 torr) = Partial pressure H2 + partial pressure of H2O.
Look in the table at 16 C and pick up the vapor pressure of water (partial pressure of water), subtract that from 752 to find the partial pressure hydrogen.

So, how do I get the grams ?

Thank you.

Again, I don't know what is in Table 5.2. Perhaps it will help. If it isn't in Table 5.2, then try using PV = nRT. You know P, V, R, and T, Calculate n = number of moles. Then mols dry gas x molar mas = grams.

I got it. Thank you so much.

To calculate the partial pressure and mass of H2, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, we need to calculate the number of moles of H2 using the ideal gas law. We know the total pressure (752 torr), the volume (1538 mL), and the temperature (16°C). However, before we proceed with the calculation, we need to convert the temperature to Kelvin and the volume to liters to match the units of the gas constant.

Converting the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 16 + 273.15
T(K) = 289.15 K

Converting the volume from milliliters to liters:
V(L) = V(mL) / 1000
V(L) = 1538 / 1000
V(L) = 1.538 L

Now, we can calculate the number of moles (n) using the ideal gas law equation, rearranged to solve for n:
n = (PV) / (RT)

Substituting the values we have:
n = (752 torr * 1.538 L) / (0.0821 L·atm/mol·K * 289.15 K)

Calculating n:
n = 19.31808 mol

Now that we have the number of moles of H2, we can calculate the partial pressure and mass of H2.

Looking at Table 5.2, we can find the molar mass of H2, which is approximately 2 g/mol.

Partial Pressure of H2:
The pressure inside the flask is the partial pressure of H2. In this case, the total pressure in the flask is the barometric pressure, which is 752 torr. Therefore, the partial pressure of H2 is also 752 torr.

Mass of H2:
The moles of H2 can be used to calculate the mass of H2 using the molar mass of H2:

Mass = moles * molar mass
Mass = 19.31808 mol * 2 g/mol

Calculating the mass of H2:
Mass = 38.63616 g

So, the partial pressure of H2 is 752 torr and the mass of H2 is 38.63616 g.