Bradley Cox
05/11/2024 · Middle School
When exposed to UV light, chlorine and hydrogen gases explosively combine to form hydrogen chloride gas. Assuming a sufficiently strong reaction vessel how much HCl (in atm) can be formed when hydrogen and chlorine are each at 5.4 atm (assume volume and temperature are constant)?
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Step-by-step Solution
To determine the amount of HCl that can be formed when hydrogen and chlorine are each at 5.4 atm, we need to consider the stoichiometry of the reaction.
The balanced chemical equation for the reaction between hydrogen (H2) and chlorine (Cl2) to form hydrogen chloride (HCl) is:
\[ \text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl} \]
From the equation, we can see that 1 mole of H2 reacts with 1 mole of Cl2 to produce 2 moles of HCl.
Given that the initial pressures of H2 and Cl2 are both 5.4 atm, we can calculate the amount of HCl that can be formed using the stoichiometry of the reaction.
Let's calculate the amount of HCl that can be formed.
Calculate the value by following steps:
- step0: Calculate:
\(2\times 5.4\)
- step1: Multiply the numbers:
\(10.8\)
The amount of HCl that can be formed when hydrogen and chlorine are each at 5.4 atm is 10.8 atm.
Quick Answer
The amount of HCl that can be formed is 10.8 atm.
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