The conversion of ammonium cyanide to urea is a second-order reaction. This means that
Chapter 3, Problem 10(choose chapter or problem)
The conversion of ammonium cyanide to urea is a second-order reaction. This means that the concentration C of ammonium cyanide at time t is given by \(1 / C=k t+1 / C_{0}\), where \(C_{0}\) is the initial concentration and k is the rate constant. Assume the initial concentration is known to be \(0.1 \mathrm{~mol} / L\) exactly. Assume that time can be measured with negligible uncertainty.
a. After 45 minutes, the concentration of ammonium cyanide is measured to be \(0.0811 \pm 0.0005 \mathrm{~mol} / L\). Estimate the rate constant k, and find the uncertainty in the estimate.
b. Use the result in part (a) to estimate the time when the concentration of ammonium cyanide will be \(0.0750 \mathrm{~mol} / \mathrm{L}\), and find the uncertainty in this estimate.
Equation Transcription:
Text Transcription:
1/C=kt + 1/C0
C0
0.1 mol/L
0.0811 \pm 0.0005 mol/L
0.0750 mol/L
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