The rate law for a hypothetical reaction is given by:

$$
\text{rate} = k [A][B]
$$

If the concentrations of $ A $ and $ B $ are both $ 0.020 \, \text{moles per liter} $ and $ k = 1.3 \times 10^{-1} \, \text{M}^{-1}\text{s}^{-1} $, what is the reaction rate?

Question

The rate law for a hypothetical reaction is given by:

$$
\text{rate} = k [A][B]
$$

If the concentrations of $ A $ and $ B $ are both $ 0.020 \, \text{moles per liter} $ and $ k = 1.3 \times 10^{-1} \, \text{M}^{-1}\text{s}^{-1} $, what is the reaction rate?

Yipes · Answer

v = 0.13\frac{L}{smol}}*0.02\frac{mol}{L}*0.02\frac{mol}{L}=5.2*10^{-5}\frac{mol}{sL}

Yipes · Answer

The reaction rate can be calculated using the rate law formula. By substituting the given values into the formula, the calculated rate is 5.2 × 1 0 − 5 mol/L/s . 
 ;

The rate law for a hypothetical reaction is given by:

\[
\text{rate} = k [A][B]
\]

If the concentrations of \( A \) and \( B \) are both \( 0.020 \, \text{moles per liter} \) and \( k = 1.3 \times 10^{-1} \, \text{M}^{-1}\text{s}^{-1} \), what is the reaction rate?

Answer (2)

The rate law for a hypothetical reaction is given by: \[ \text{rate} = k [A][B] \] If the concentrations of \( A \) and \( B \) are both \( 0.020 \, \text{moles per liter} \) and \( k = 1.3 \times 10^{-1} \, \text{M}^{-1}\text{s}^{-1} \), what is the reaction rate?

Answer (2)

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The rate law for a hypothetical reaction is given by:

\[
\text{rate} = k [A][B]
\]

If the concentrations of \( A \) and \( B \) are both \( 0.020 \, \text{moles per liter} \) and \( k = 1.3 \times 10^{-1} \, \text{M}^{-1}\text{s}^{-1} \), what is the reaction rate?