how many liters of hydrogen gas can be formed at 722 mmHg at 15 degress C when 5.5 grams of zinc metal with 150 mL of 1.25 molarity HCl solution?

I got 2.09 L of Hydrogen gas, but I am not sure if that is correct. Can anyone confirm?

I agree with 2.09L. Good work. This is a limiting reagent problem; it's good you recognized that.

To find out how many liters of hydrogen gas can be formed, 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 ideal gas constant, and T is the temperature.

First, let's calculate the number of moles of zinc (Zn) using its molar mass. The molar mass of zinc is 65.38 g/mol.

Number of moles of Zn = Mass of Zn / Molar mass of Zn
= 5.5 g / 65.38 g/mol
≈ 0.0841 mol

Next, we need to calculate the number of moles of hydrogen gas (H2) formed. From the balanced chemical equation, we know that 1 mole of zinc reacts with 2 moles of HCl to produce 1 mole of H2.

Number of moles of H2 = Number of moles of Zn × 1 mole of H2 / 1 mole of Zn
= 0.0841 mol × 1 mol / 1 mol
= 0.0841 mol

The volume of the gas can be determined by rearranging the ideal gas law equation and solving for V:

V = nRT / P

Given:
Pressure (P) = 722 mmHg
Temperature (T) = 15 °C

First, let's convert the pressure to atmospheres (atm) since the ideal gas constant (R) is given in atm.

1 atm = 760 mmHg

Pressure (P) = 722 mmHg / 760 mmHg/atm
≈ 0.95 atm

The ideal gas constant (R) is 0.0821 L·atm/(mol·K).

Now, let's convert the temperature from Celsius to Kelvin (K):

Temperature (T) in Kelvin = 15 °C + 273.15
= 288.15 K

Now, we can substitute the values into the ideal gas law equation:

V = (0.0841 mol) × (0.0821 L·atm/(mol·K)) × (288.15 K) / (0.95 atm)
≈ 2.568 L

Therefore, approximately 2.568 liters of hydrogen gas can be formed at 722 mmHg and 15 degrees Celsius when 5.5 grams of zinc metal react with 150 mL of 1.25 molarity HCl solution.