If Co=0.2, ke=0.14 hr 1, k=2.0*10^6 and [C] at t=0 is 1.5*10*6, What will be the [C] at t=4 hr. Assume d[C]/dt=-kC and C follows a first order clearance Give the correct answer only

The concentration \([C]\) at \( t = 4 \) hours is approximately \( 0 \). 

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Here are 5 related questions:
1. What is the half-life in a first-order reaction?
2. How does the rate constant \(k\) affect the clearance rate?
3. What happens to the concentration if \(t\) increases in a first-order process?
4. Can a first-order reaction have a constant clearance rate?
5. How would changing the initial concentration \([C_0]\) affect the outcome?

**Tip:** First-order reactions have an exponential decay, meaning concentration decreases rapidly with time.

If Co=0.2, ke=0.14 hr⁻¹, k=2.0*10^6 and [C] at t=0 is 1.5*10^6, What will be the [C] at t=4 hr. Assume d[C]/dt=-kC and C follows a first order clearance.

Learn how to solve a first-order clearance problem where Co=0.2, ke=0.14 hr⁻¹, k=2.0*10^6, and [C] at t=0 is 1.5*10^6. This detailed explanation covers differential equations, exponential decay, and first-order kinetics. Suitable for undergraduate-level chemistry and applied mathematics.

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