Alaboratory assistant needs to prepare 35.2 liters of hydrogen at 25.0°c and 101.3 kilopascals. this is the equation for the reaction: 2hcl + ca → h2 + cacl2 what volume of 2.3 m hydrochloric acid is required to produce this much gas? use the ideal gas resource. a. 0.625 l b. 0.876 l c. 1.18 l d. 1.25 l (some chart that i don't understand)

Option A= 0.625 L

Explanation:

Given data:

Volume of hydrogen =35.2 L

Temperature = 25 °C = 25 + 273 = 298 K

Pressure = 101.3 Kpa = 0.99975327 atm

Molarity of HCl = 2.3 mol / L

Volume of HCl require = ?

Solution:

Formula:

PV = nRT

n = PV / RT

n = (0.99975327 atm × 35.27 L) / 0.0821 atm. L/ mol.K × 298 k

n = 35.19 atm . L / 24.4658 L. atm /mol

n = 1.438 mol

we know that molarity is equal to:

Molarity = number of moles / volume in liter

Volume in liter = Number of moles / Molarity

Volume in liter = 1.438 mol / 2.3 mol/ L

Volume in liter = 0.625 L