Question

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 = kt + 1/C0, where C0 is the initial concentration and k is the rate constant. Assume the initial concentration is known to be 0.1 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 ? 0.0005 mol/L. Estimate the rat? 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 mol/L, and find the uncertainty in this estimate.

Answer 1

The conversion of ammonium cyanide to urea is a second-order reaction. We can estimate the rate constant k and find the uncertainty by plugging in the values of C and C0. We can also estimate the time required for the concentration to reach a specific value using the rate constant.

Step-by-step explanation:

The given equation 1/C = kt + 1/C0 represents a second-order reaction where C is the concentration of ammonium cyanide at time t, C0 is the initial concentration, and k is the rate constant.

To estimate the rate constant k, we can rearrange the equation to find C at time t. Plugging in the values C0 = 0.1 mol/L and C = 0.0811 mol/L at t = 45 minutes, we can solve for k.

Once we have the value of k, we can use the equation to estimate the time required for the concentration to reach 0.0750 mol/L. By plugging in the values of C0, C, and k into the equation and solving for t, we can determine the time and find the uncertainty in this estimate.