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Chemistry Help Hey guys I need help with this chemistry problem. Consider the following hypothetical aqueous reaction: A-->B. A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 Part A) By using appropriate graphs, determine whether the reaction is first order or second order. Part B) What is the rate constant for the reaction? Part C) What is the half-life for the reaction? If you guys could show work I would be grateful. Thank you

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