Question

Given the following balanced equation, determine the rate of reaction with respect to [NOCl].

2NO(g) + Cl2(g) → 2NOCl(g)
It is not possible to determine the answer without more information.

Answer 1

The rate of reaction with respect to
`\([NOCl]\)` at that particular moment is
`\(-0.04 \, \text{M/s}\)`. The negative sign indicates the consumption of NOCl.

To answer this question, we need to use the information given in the statement about the rate of reaction with respect to
`\([NOCl]\)` . The statement is:

`\[ \text{Rate} = (1)/(2)(\Delta [NOCl])/(\Delta t) \]`

The given information is that the concentration of NO is changing at a rate of
`\(-0.02 \, \text{M/s}\),`and the balanced equation is
`\(2NO(g) + Cl_2(g) \rightarrow 2NOCl(g)\).`

Since the coefficient of NOCl is 2 in the balanced equation, the rate of formation of NOCl
`(\((\Delta [NOCl])/(\Delta t)\))` is twice the rate of change of NO
`(\((\Delta [NO])/(\Delta t)\)).`

Therefore, the rate of formation of NOCl is
`\(2 * (-0.02 \, \text{M/s}) = -0.04 \, \text{M/s}\).`

So, the rate of reaction with respect to
`\([NOCl]\)` at that particular moment is
`\(-0.04 \, \text{M/s}\).` The negative sign indicates the consumption of NOCl.

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The probable question maybe:

If the concentration of NO is changing at a rate of
`\(-0.02 \, \text{M/s}\) in a reaction described by the equation \(2NO(g) + Cl_2(g) \rightarrow 2NOCl(g)\),`what is the rate of reaction with respect to \([NOCl]\) at that particular moment?

This question allows you to use the given statement about the rate of reaction with respect to \([NOCl]\) and apply it to a specific scenario where the concentration of NO is changing. The rate of reaction with respect to \([NOCl]\) would be the positive value corresponding to the rate of formation of NOCl.