QuestionJuly 24, 2025

2N_(2)O_(5)(aq)arrow 4NO_(2)(aq)+O_(2)(g) In a previous step, you calculated the rate of disappearance of N_(2)O_(5) at 5.0times 10-4M/s What is the rate of appearance of NO_(2) in the same timeframe? Rate=-(1)/(2)(Delta [N_(2)O_(5)])/(Delta t)=(1)/(4)(Delta [NO_(2)])/(Delta t) Rate_(O_(2))=[?]times 10^[?]M/s Coefficient (green) Exponent (yellow)

2N_(2)O_(5)(aq)arrow 4NO_(2)(aq)+O_(2)(g) In a previous step, you calculated the rate of disappearance of N_(2)O_(5) at 5.0times 10-4M/s What is the rate of appearance of NO_(2) in the same timeframe? Rate=-(1)/(2)(Delta [N_(2)O_(5)])/(Delta t)=(1)/(4)(Delta [NO_(2)])/(Delta t) Rate_(O_(2))=[?]times 10^[?]M/s Coefficient (green) Exponent (yellow)
2N_(2)O_(5)(aq)arrow 4NO_(2)(aq)+O_(2)(g) In a previous step, you calculated the rate of disappearance of N_(2)O_(5) at 5.0times 10-4M/s What is the rate of appearance of NO_(2) in the same timeframe? Rate=-(1)/(2)(Delta [N_(2)O_(5)])/(Delta t)=(1)/(4)(Delta [NO_(2)])/(Delta t) Rate_(O_(2))=[?]times 10^[?]M/s Coefficient (green) Exponent (yellow)

Solution
4.4(387 votes)

Answer

1.0 \times 10^{-3} M/s Explanation 1. Identify the relationship between rates Use the stoichiometry of the reaction. The rate of disappearance of N_{2}O_{5} is related to the rate of appearance of NO_{2} by their coefficients in the balanced equation. 2. Apply the rate formula Given Rate = -\frac{1}{2}\frac{\Delta [N_{2}O_{5}]}{\Delta t} = \frac{1}{4}\frac{\Delta [NO_{2}]}{\Delta t}, solve for \frac{\Delta [NO_{2}]}{\Delta t} using the given rate of disappearance of N_{2}O_{5}, which is 5.0 \times 10^{-4} M/s. 3. Calculate the rate of appearance of NO_{2} Rearrange the formula: \frac{\Delta [NO_{2}]}{\Delta t} = 4 \times \left(-\frac{1}{2}\frac{\Delta [N_{2}O_{5}]}{\Delta t}\right). Substitute the given rate: \frac{\Delta [NO_{2}]}{\Delta t} = 4 \times (5.0 \times 10^{-4} M/s).

Explanation

1. Identify the relationship between rates<br /> Use the stoichiometry of the reaction. The rate of disappearance of $N_{2}O_{5}$ is related to the rate of appearance of $NO_{2}$ by their coefficients in the balanced equation.<br /><br />2. Apply the rate formula<br /> Given $Rate = -\frac{1}{2}\frac{\Delta [N_{2}O_{5}]}{\Delta t} = \frac{1}{4}\frac{\Delta [NO_{2}]}{\Delta t}$, solve for $\frac{\Delta [NO_{2}]}{\Delta t}$ using the given rate of disappearance of $N_{2}O_{5}$, which is $5.0 \times 10^{-4} M/s$.<br /><br />3. Calculate the rate of appearance of $NO_{2}$<br /> Rearrange the formula: $\frac{\Delta [NO_{2}]}{\Delta t} = 4 \times \left(-\frac{1}{2}\frac{\Delta [N_{2}O_{5}]}{\Delta t}\right)$. Substitute the given rate: $\frac{\Delta [NO_{2}]}{\Delta t} = 4 \times (5.0 \times 10^{-4} M/s)$.
Click to rate:

Similar Questions