Count the significant digits in each of these measurements: measurement 0.003600 J number of significant digits -2 - 8.0 x 10 kJ/mol 51800. kg 9.9 x 10 -1 mL G

One student calibrated a 50-ml burette by using the mass of water delivered. The student used an analytical balance which was previously calibrated by STEEL (density = 7.8 g/mL). During calibration, the temperature of water was found to be 19.0.C. The density of water at this temperature is 0.9984 g/ml The results of the calibration by the student is shown in the table below:   A B C  D E Apparent burette reading,mL 10.05 20.04 30.08 40.07 49.98 Weight H2O delivered, g 10.03 20.09 30.05 40.02 49.83 Note: All masses in mentioned in this section are understood to be in grams and all volumes mentioned are understood to be in milliliters. 35. What is the true mass of water delivered in A? A) 10.03 B) 10.04 C) 10.05 D) 10.06 E) 10.07 36. What is the true mass of water delivered in B? A) 20.12 B) 20.13 C) 20.14 D) 20.15 E) 20.1637. What is the true mass of water delivered in C? A) 30.13 B) 30.11 C) 30.10 D) 30.09 E) 30.08 38. What is the true mass of water delivered in D? A) 40.09…

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© Macmillan Learning Perform the calculation and report the answer using the proper number of significant figures. Make sure the answer is rounded correctly. 1.012 × 10-³ J = (0.016456 g) (298.3682 298.3567) K g. K