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24 Mar 2020
Urea (NH2CONH2) is the end product in protein metabolism in animals. The decomposition of urea in 0.1 M HCl occurs according to the reaction
NH2CONH2(aq) + H+(aq) + 2 H2O(l)
2 NH4+(aq) + HCO3-(aq)
The reaction is first order in urea and first order overall. When [NH2CONH2] = 0.200 M, the rate at 61.05 °C is 8.56 × 10-5 M/s. (a) What is the rate constant, k? (b) What is the concentration of urea in this solution after 4.00 × 103 s if the starting concentration is 0.500 M? (c) What is the halflife for this reaction at 61.05 °C?
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b) The integrated rate law for the first order reaction
![](data:image/png;base64,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)
can be used for calculation of the amount of substrate remained after any time period.
In this case,
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![](data:image/png;base64,iVBORw0KGgoAAAANSUhEUgAAAHEAAAAOBAMAAADqJO73AAAACXBIWXMAAABkAAAAZAAPlsXdAAAAKlBMVEUAAAAAAABHcEwAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAACqYB4GAAAADXRSTlOIRAC7MyJmVRHMoud3LiHs4gAAAWlJREFUKM+V0s9LAkEUB/BxTkEF7lqSnma/+9PQgxKebaGTBBLUoS4iUYQdooLKPNT+B21R15TAu/UPFHjrP4j+l96smeu6Bb3Dziy8z7x5M8MwDGcRk2Es4c8QLKkGk/wgKl+judfB1wRUODAFE3y4hBpNVCL/1n5ZDjm0k654vvmHrOFSDgfwnb69501Lx4W5ESfXvQLlmCmthDtN9il4ppf1SGZ4U7lv4j3rJVpejERQ09ZFCUVbmZFSdHWVpOC6yjTNt/iLeBvKGqMYS9nneSANnASSjyVEJ82tFkc3XLNOC1BKgzbrBhIo1KYkh1MUfOtJyisScz/+jPq32CyjPqsoVMIyR1Lz0S6JxPZASk1RlIUR1Fwbp1TM8dGvoCpYqpgqNjskzc5F77aBenrz4ai87E2d0M7nBx5hzicO88f5tRUxOgC6FcMJZq58JroRc7bfYdJDXfXCMhz67u9y9G7jZex9TsovySqAv0oxFZIAAAAASUVORK5CYII=)
![](data:image/png;base64,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)
c) The half-life for the first order reaction is
![](data:image/png;base64,iVBORw0KGgoAAAANSUhEUgAAAR8AAAAeBAMAAADnUgdvAAAACXBIWXMAAABkAAAAZAAPlsXdAAAAJ1BMVEVHcEwAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAB+jSoGAAAADHRSTlMAiERsETNVIrjnzJlLmmG+AAAD0klEQVRYw7VXzU8TQRT/bXd2ty0ctnxKwqFVEfw4LKAoelnRxA88bK1RiR4WUAJ6qZio8dTg53GJHD3ggXjwQoRgvCkx8eIf5XszLbR0uza1+5rM7uzMzvz63pvf+y0QarmsvJyGyEJ3EWlyqvDkzRRiMs3n1sxifNERduTU+RxhQd8sRnNeYu5VTIDS0itJWLYZ4Ezk1HUR0B9wZqzAKnV6SzEBui7bPIxf2KVLhCVK2ABuAHoJv033XEyARq0LC7OY4LAF5Kio4JawApw40k+AdiHexARox0xlr6KLw+Yg/W9AA8WXIjB2UeiNCdCaeIlF3gndaMZDk+jM5h/uAktuLHisdYxiiz1k+s+jPWTKHDpBgCCCe7ifbXHLZ37kLv3eDgKfAA3Bj/aQWEdgeimk3He6PemeKrbogs3HUcPGFtaw4uVhffwT4EnkUuO6n7TNb1t4fRLarWgeEmUOFdV+pCAnAG+00r8d9maRfpcrronmIWuY2+Uipoggb0Y6yJiE4lCi272HhQDmWC+HvmzdEZFTf2SzbbnZCcWhTLd79oOS9BowUul/jljgtDxHblsBEYdKuoUGXFKARpAuODyGoy5mVyPOhcHNFbQVEHGopFsYtthWgA4hOXyWI1WYKsFUpdOS7ZMMWehSjUeaOUL8sl0GRBwq6ZYq07S7Byib4Ps+OFzXDcpEzarOpVymxuyGI01Y1wEPMYeqxE2sYR+QvJ354nJdv0C9wlOdtr1IC/Dc5cM1lm040oTRIRQMzKmEjAAx3QLTuTKgRaQ9xQD5EtKJokYb2rOgsCZogaHwot5wpBljYJ4EpDiU6RZi27AVoOtIVQ5RCck5ECASYbrdnsStPiNGLS3pg92SQyXd8uktsLD46ejOhJqQOeZDFBmQXgxRPSI0izn9mWkTBxi4DMSqYhiZDHW2XGz4yFVXAqTB8OtfHgkVk1wuFh1zbryGgZWSlTqtSgq0Vmrv9pPvZt6X6mVa2OzzkMJWQ0fN6ZFKlsxvAyCy8PxZCYvYiGLalNch3xPq9LCS1TOZPsMrA+JO64AafFgE8+v19U1WXPLQz16puiW5dZZ1GmVWZpXyQJ9z/s9DVmiRNt7eceoePpCAko74vsFTerZRAwjGB0L4Qh1oToZ2mv4pBLqXVBJhWgywb467BwBJuxbP51lyqD7P9cyAErYT6KB4iK+2AqSU7F4KPHLiAJQiFRtWsU2PmHYeGsV52s2rZ6xk92MdmLEAuosdrz5mg13JfmJazV+gXg8MRzIwK9l9B43NxxIyURYl4XZArSolW3FR65ruL2AXs9WDjJmoAAAAAElFTkSuQmCC)
Urea (NH2CONH2) is the end product in protein metabolism in animals. The decomposition of urea in 0.1 M HCl occurs according to the reaction
NH2CONH2(aq) + H+(aq) + 2 H2O(l) 2 NH4+(aq) + HCO3-(aq)
The reaction is first order in urea and first order overall. When [NH2CONH2] = 0.200 M, the rate at 61.05 °C is 8.56 × 10-5 M/s. (a) What is the rate constant, k? (b) What is the concentration of urea in this solution after 4.00 × 103 s if the starting concentration is 0.500 M? (c) What is the halflife for this reaction at 61.05 °C?
b) The integrated rate law for the first order reaction
can be used for calculation of the amount of substrate remained after any time period.
In this case,
c) The half-life for the first order reaction is
Jarrod RobelLv2
20 May 2020