Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. BrNO(g) + NO(g) → 2 BrNO(g) Δ[Br,NO] Δt a. b. Δ[Br,NO] Δt Δ[Br,NO] Δt Δ[Βr,NO] Δt 2 = Δ[HOF] ΔΕ Δ[ΝΟ] 1 Δt 2 Δ[HOF] At Δ[HF] ΔΕ Δ[ΝΟ] Δt Δ[ΝΟ] ΔΕ Δ[ΝΟ] Δt 2 HOF(g) → 2 HF(g) + O2(g) Δ[HOF] Δ[02] Δ[HF] Δt Δt ΔΕ = = Δ[02] Δt 1 /Δ[BrNO] ΔΕ Δ[02] Δt Δ[02] Δt 1 Δ[BrNO] 2 Δt || = = Δ[BrNO] Δt 12 Δ[BrNO] Δt 2 1 2 1 2 Δ[HF] ΔΕ Δ[HF] ΔΕ Δ[HOF] Δt
Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. BrNO(g) + NO(g) → 2 BrNO(g) Δ[Br,NO] Δt a. b. Δ[Br,NO] Δt Δ[Br,NO] Δt Δ[Βr,NO] Δt 2 = Δ[HOF] ΔΕ Δ[ΝΟ] 1 Δt 2 Δ[HOF] At Δ[HF] ΔΕ Δ[ΝΟ] Δt Δ[ΝΟ] ΔΕ Δ[ΝΟ] Δt 2 HOF(g) → 2 HF(g) + O2(g) Δ[HOF] Δ[02] Δ[HF] Δt Δt ΔΕ = = Δ[02] Δt 1 /Δ[BrNO] ΔΕ Δ[02] Δt Δ[02] Δt 1 Δ[BrNO] 2 Δt || = = Δ[BrNO] Δt 12 Δ[BrNO] Δt 2 1 2 1 2 Δ[HF] ΔΕ Δ[HF] ΔΕ Δ[HOF] Δt
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Understanding Reaction Rates
This section focuses on the relative rates of disappearance of reactants and the formation of products for given chemical reactions.
**Reaction a:**
\[ \text{Br}_2\text{NO(g)} + \text{NO(g)} \rightarrow 2 \text{BrNO(g)} \]
- **Options for Rate Expressions:**
1. \[ -\frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = -\frac{\Delta[\text{NO}]}{\Delta t} = \frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
2. \[ \frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = \frac{\Delta[\text{NO}]}{\Delta t} = -\frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
3. \[ \frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = \frac{\Delta[\text{NO}]}{\Delta t} = \frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
4. \[ -\frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = -\frac{\Delta[\text{NO}]}{\Delta t} = \frac{\Delta[\text{BrNO}]}{\Delta t} \]
**Reaction b:**
\[ 2 \text{HOF(g)} \rightarrow 2 \text{HF(g)} + \text{O}_2\text{(g)} \]
- **Options for Rate Expressions:**
1. \[ \frac{\Delta[\text{HOF}]}{\Delta t} = \frac{\Delta[\text{O}_2]}{\Delta t} = \frac{\Delta[\text{HF}]}{\Delta t} \]
2. \[ -\frac{1}{2} \left( \frac{\Delta[\text{HOF}]}{\Delta t} \right) = \frac{\Delta[\text{O}_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd32c0099-d35b-45af-b7af-24c06e9e82b9%2Fed6d26f4-2af0-4f88-a706-e3f635a78076%2Fx8hjdxq_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Reaction Rates
This section focuses on the relative rates of disappearance of reactants and the formation of products for given chemical reactions.
**Reaction a:**
\[ \text{Br}_2\text{NO(g)} + \text{NO(g)} \rightarrow 2 \text{BrNO(g)} \]
- **Options for Rate Expressions:**
1. \[ -\frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = -\frac{\Delta[\text{NO}]}{\Delta t} = \frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
2. \[ \frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = \frac{\Delta[\text{NO}]}{\Delta t} = -\frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
3. \[ \frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = \frac{\Delta[\text{NO}]}{\Delta t} = \frac{1}{2} \left( \frac{\Delta[\text{BrNO}]}{\Delta t} \right) \]
4. \[ -\frac{\Delta[\text{Br}_2\text{NO}]}{\Delta t} = -\frac{\Delta[\text{NO}]}{\Delta t} = \frac{\Delta[\text{BrNO}]}{\Delta t} \]
**Reaction b:**
\[ 2 \text{HOF(g)} \rightarrow 2 \text{HF(g)} + \text{O}_2\text{(g)} \]
- **Options for Rate Expressions:**
1. \[ \frac{\Delta[\text{HOF}]}{\Delta t} = \frac{\Delta[\text{O}_2]}{\Delta t} = \frac{\Delta[\text{HF}]}{\Delta t} \]
2. \[ -\frac{1}{2} \left( \frac{\Delta[\text{HOF}]}{\Delta t} \right) = \frac{\Delta[\text{O}_
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