In 6 M HCl, the complex ion Ru(NH₃)₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃)₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃)₆³⁺] to decrease to 39.0% of its initial value?

Question

Quizplus · Accepted Answer

For a first-order reaction, the time to reach a certain percentage of the initial concentration can be calculated using the formula: t = (t₁/₂ / 0.693) * ln(1 / fraction remaining). Here, t₁/₂ = 14 h and fraction remaining = 0.39. Calculating gives t ≈ 19 h.

In 6 M HCl, the Complex Ion Ru(NH3)63+ Decomposes to a Variety

In 6 M HCl, the Complex Ion Ru(NH₃)₆³⁺ Decomposes to a Variety