Question

A laboratory 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.

Answer 1

The ideal gas equation states that the volume is directly proportional to the moles and temperature but inversely to pressure. The volume required is 1.25 L.

What is the ideal gas equation?

An ideal gas is the hypothetical gas equation that depicts the relation of the temperature, pressure, volume and moles of the substance of the gas.  It is given as,

$\rm PV = nRT$

Where,

The pressure of hydrogen gas (P) = 1 atm

The volume of hydrogen gas (V) = 35.2L

The temperature of hydrogen gas (T) = 298 K

Gas constant (R) = 0.0821 L. atm. per mol. per K

Substituting values in the equation,

$\begin{aligned}\rm n &= \rm \dfrac{PV}{RT}\\\\&= \dfrac{35.2\times 1}{0.0821\times 298}\\\\&= 1.438\;\rm moles\end{aligned}$

The balanced chemical reaction can be shown as,

$\rm 2HCl + Ca \rightarrow H_{2} + CaCl_{2}$

From the reaction, it can be deduced that, 2 moles of hydrochloric acid = 1 mole of hydrogen gas.

So, 1.438 moles of hydrogen molecules will produce 2.876 moles of HCl.

The volume of HCl can be calculated as,

$\begin{aligned}\rm Volume &= \rm \dfrac{moles}{Molarity}\\\\&= \dfrac{2.876}{2.3}\\\\&= 1.25\end{aligned}$

Therefore, option D. 1.25 L is the volume of the hydrochloric acid.

Learn more about volume and molarity here:

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