Step-by-step explanation:
To determine the number of molecules of hydrochloric acid (HCl) needed to produce 1.50 liters of hydrogen gas (H2) in the given reaction, we need to first convert the volume of hydrogen gas to the number of moles using the ideal gas law, and then use the balanced chemical equation to determine the stoichiometry between HCl and H2.
Step 1: Convert liters of hydrogen gas to moles using the ideal gas law.
The ideal gas law is given by:
PV = nRT
where:
P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant
T = temperature of the gas
Since the pressure, temperature, and ideal gas constant are not provided in the question, we cannot perform this conversion without this information.
Step 2: Use the balanced chemical equation to determine the stoichiometry between HCl and H2.
The balanced chemical equation for the reaction between hydrochloric acid (HCl) and zinc (Zn) is:
2 HCl + Zn → ZnCl2 + H2
From the balanced chemical equation, we can see that 2 moles of HCl are required to produce 1 mole of H2.
Step 3: Multiply the stoichiometric ratio between HCl and H2 by the number of moles of H2 calculated in step 1 to find the number of moles of HCl needed.
Since we cannot perform step 1 without the necessary information, we cannot accurately determine the number of molecules of hydrochloric acid needed to produce 1.50 liters of hydrogen gas. We would need to know the pressure, temperature, and ideal gas constant in order to perform the conversion from liters to moles and determine the required amount of HCl