Use the following equation and graph to answer questions 1 and 2. Hydrogen iodide decomposes at 410 °C, according the reaction: 2 HI1g2¡H21g2 + I21g2 The graph shows how the concentration of HI changes over time. What is the average rate of loss of HI over the time period 0–40 s (LO 14.1) (a) 7.5 * 10-3 M>s (b) 4.8 * 10-3 M>s (c) 3.0 * 10-2 M>s (d) 3.5 * 10-3 M>s

Video transcript

Hello everyone today we are being asked the following question. The graph below shows the time dependent change in the concentration of nitric oxide. If nitric oxide decomposes at 520°C based on the following equation, what is the average rate of consumption of nitric oxide over the time interval 0-20 seconds. So it's important to recall that the rate of a reaction is given by the phone equation. The rate is equal to we have negative one over A. Which is our first variable times to change in the concentration of our A. Over the time. And this can be equal to one over B. Or secondary times. The concentration of our secondary reacted over the change in time. So this simplifies to the equation we have our rate is equal to our change in our concentration of A. Over our change in our time. And so we're going from 0 to 20 seconds. We can note That when T. is equal to 20 The concentration for our nitric oxide is 0.35. And when T equals zero the concentration of nitric oxide is equal to 0.45. And so plugging it into our equation, we get 0.35 minus point 45/20 minus zero. And this is going to simplify to negative five, discount the negative. It's just going to simplify to negative 0.5 or 5.0 times 10 to the negative third molar per second. And so this is going to be our final answer overall. I hope this helped. And until next time