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- What is the uncertainty, in terms of a power of 10, associated with each of the following measured values? a. 4.30 102 b. 4.300 101 c. 4.3 103 d. 4.300 105In the pairs of numbers of Problem 2-34, tell whether both members of the pair have the same uncertainty. a. 345,000 and 340,500 b. 2302 and 2320 c. 0.6600 and 0.66 d. 936 and 936,000A measurement of the mass of a specimen was determined to be 4.203 plus or minus 0.001 g. What is the fractional uncertainty in the mass?
- The density of an irregular shaped object was measured three times with the following results: 2.15 g/cm3 2.79 g/cm3 1.98 g/cm3 How would you report the mean and standard deviation of this data? a. 2.31 g/cm3 ± 0.07 g/cm3 b. 2.307 g/cm3 ± 0.1 g/cm3 c. 2.4 g/cm3 ± 0.5 g/cm3 d. 2.15 g/cm3 ± 0.03 g/cm3 e. 2.3 g/cm3 ± 0.4 g/cm3The answer isn’t 0.0011, 0.0055, or 0.0071Straight-chain, saturated carboxylic acids, a class of hydrocarbons, has the general formula CnH2n+1COOH where n is an integer than ranges from 1 to 18. What would be the %C by mass if n = 1 ? Atomic weights: C=12.01, H=1.01, O=15.99. Input values only with 2 decimal places. Do not include the units.
- Please show the calculation in B. Where the final answer is 2800.6 JStraight-chain, saturated carboxylic acids, a class of hydrocarbons, have the general formula CnH2n+1COOH where n is an integer that ranges from 1 to 18. What would be the %C by mass if n = 8? Atomic weights: C = 12.01, H = 1.01, O = 15.99. Input values only with two decimal places. Do not include the units.What is the result of the following calculation to the correctnumber of significant figures?(6.266 − 6.261) ÷ 522.0 = a) 9.5785 × 10–6b) 9.579 × 10–6c) 9.58 × 10–6d) 9.6 × 10–6e) 1 × 10–5
- What is the uncertainty in the measured value 12.37040 after it is rounded to the following number of significant figures? The uncertainty of 6 is? The uncertainty of 4 is? The uncertainty of 3 is?A group of students took turns using a laboratory balanceto weigh the water contained in a beaker. The results theyreported were 111.42 g, 111.67 g, 111.21 g, 135.64 g,111.02 g, 111.29 g, and 111.42 g.(a) Should any of the data be excluded before the average is calculated?(b) From the remaining measurements, calculate the average value of the mass of the water in the beaker.(c) Calculate the standard deviation s and, from it, the 95% confidence limit.The standard solution is prepared by dissolving a known mass of zinc pellets with conc. HCl. The solution is then neutralized, transferred into a 250 mL volumetric flask and filled to the calibration mark. If 0.9809 g of Zn was weighed using an electronic balance with a relative uncertainty of ± 0.01 % and the 250 mL volumetric flask has a known relative uncertainty of ± 0.06 %, what would be the absolute uncertainty of the concentration of the solution? The molecular weight of the zinc pellets is 65.39 g/mol