Final answer:
Option D (3.65 g/ml) is the only accurate value in the set given the accepted density value. The accuracy and significant figures principle dictates that the recorded data should match the precision of the accepted value, which in this case is three significant figures.
Step-by-step explanation:
The student has asked if a set of density data is accurate given that the accepted value is 3.65 g/ml. To determine the accuracy of the data, we need to compare the given values with the accepted density. The best representation of an accurate measurement from the options given is option D, which is precisely the accepted value of 3.65 g/ml.
When considering significant figures, we note that the accepted value has three significant figures. Therefore, any measured values should also be presented with the same level of precision. For instance, if we find a value of 0.866728... g/mL in a calculation, the result should be rounded to three significant figures, giving us 0.867 g/mL. Similarly, if we have a density of 7.80 g/cm³, calculated from numbers with three significant figures like 23.4 and 3.00, we ensure our answer matches the precision level with three significant figures, 7.80.
Lastly, when measurements with different levels of precision are involved in a calculation, the answer must match the least precise measurement. For example, in a multiplication 0.638 x 6.6 mL, we have to round our answer to one decimal place because 6.6 mL has only one decimal place. Accuracy and significant figures play a crucial role in properly reporting and interpreting scientific data.