An investigator monitored the rate of reaction between calcium carbonate granules and dilute nitric acid by measuring the total mass loss as carbon dioxide gas escaped from the reaction vessel.
The table below shows the mass of the flask and its contents recorded at regular intervals:
Time (s)Mass of flask and contents (g)0180.0040178.2080176.80120175.80160175.00200174.40240174.00280174.00\begin{array}{|c|c|} \hline \text{Time (s)} & \text{Mass of flask and contents (g)} \\ \hline 0 & 180.00 \\ \hline 40 & 178.20 \\ \hline 80 & 176.80 \\ \hline 120 & 175.80 \\ \hline 160 & 175.00 \\ \hline 200 & 174.40 \\ \hline 240 & 174.00 \\ \hline 280 & 174.00 \\ \hline \end{array}Time (s)04080120160200240280Mass of flask and contents (g)180.00178.20176.80175.80175.00174.40174.00174.00
Calculate the mean rate of reaction between 0 seconds0\text{ seconds}0 seconds and 200 seconds200\text{ seconds}200 seconds.
Use the equation: mean rate of reaction=mass of gas losttime taken\text{mean rate of reaction} = \frac{\text{mass of gas lost}}{\text{time taken}}mean rate of reaction=time takenmass of gas lost
State the value and choose the correct unit from: g/s\text{g/s}g/s, s/g\text{s/g}s/g, g/s2\text{g/s}^2g/s2, or s/g2\text{s/g}^2s/g2.