Question

question 6 (1 point)
give the theoretical rate equation for the forward direction when all are gases in a closed container.
$\ce{c2h6 + 2 cl2 <=> c2h4cl2 + 2 hcl}$
the rate requires the collision - interactions of 1 $\ce{c2h6}$, 2 $\ce{cl2}$, and 3 $\ce{c2h4cl2}$ molecules.
this is also reflected as the exponents in the rate equation,
$\text{rate}^f = k^f __4__ __5__^2$
a. $\ce{c2h6}$ b. $\ce{cl2}$ c. $\ce{c2h4cl2}$ d. $\ce{hcl}$ e. 1 f. 2 g. 3 h. 4
i. 5 j. 6 k. 7 l. 8 m. 9 n. 10 o. 0 p. $\ce{ph3}$ q. $\ce{h2}$
r. $\ce{o2}$ s. $\ce{p2o5}$ t. $\ce{h2o}$ u. 25

Explanation:

Step1: Analyze Collision Interactions

The reaction is \( \ce{C2H6 + 2Cl2 <=> C2H4Cl2 + 2HCl} \). For the forward rate, the collision involves 1 \( \ce{C2H6} \), 2 \( \ce{Cl2} \), and 0 \( \ce{C2H4Cl2} \) (since \( \ce{C2H4Cl2} \) is a product, not a reactant in forward direction). So:

• 1: E (1) (number of \( \ce{C2H6} \) molecules)
• 2: F (2) (number of \( \ce{Cl2} \) molecules)
• 3: O (0) (number of \( \ce{C2H4Cl2} \) molecules, as it's a product)

Step2: Determine Rate Equation Components

The rate equation for forward reaction depends on reactants. Reactants are \( \ce{C2H6} \) and \( \ce{Cl2} \). The exponents match the stoichiometry (1 for \( \ce{C2H6} \), 2 for \( \ce{Cl2} \)). So:

• 4: A (\( \ce{C2H6} \))
• 5: B (\( \ce{Cl2} \))

Answer:

1: E. 1
2: F. 2
3: O. 0
4: A. \( \ce{C2H6} \)
5: B. \( \ce{Cl2} \)