(a)
Interpretation: The fixed notation and correct number of significant figure has to be expressed.
Concept introduction:
Scientific notation expression: A number is expressed as the product of two numbers:
Significant of zeroes:
- Zeroes between two other significant digits are significant.
- Zeroes to the right of a nonzero number, and also to the right of decimal place, are significant.
- Zeroes that are placeholders are not significant.
(b)
Interpretation: The fixed notation and correct number of significant figure has to be expressed.
Concept introduction:
Scientific notation expression: A number is expressed as the product of two numbers:
Significant of zeroes:
- Zeroes between two other significant digits are significant.
- Zeroes to the right of a nonzero number, and also to the right of decimal place, are significant.
- Zeroes that are placeholders are not significant.
(c)
Interpretation: The fixed notation and correct number of significant figure has to be expressed.
Concept introduction:
Scientific notation expression: A number is expressed as the product of two numbers:
Significant of zeroes:
- Zeroes between two other significant digits are significant.
- Zeroes to the right of a nonzero number, and also to the right of decimal place, are significant.
- Zeroes that are placeholders are not significant.
(d)
Interpretation: The fixed notation and correct number of significant figure has to be expressed.
Concept introduction:
Scientific notation expression: A number is expressed as the product of two numbers:
Significant of zeroes:
- Zeroes between two other significant digits are significant.
- Zeroes to the right of a nonzero number, and also to the right of decimal place, are significant.
- Zeroes that are placeholders are not significant.
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Chemistry & Chemical Reactivity
- For each of the following numbers, determine the number ofsignificant figures it contains, rewrite it without using scientific notation, and determine thenumber of significant figures in the result. (a) 3.050 × 10–4 , (b) 4.3200 × 102 , (c) 8.001 × 10–7, (d) 2.006080 × 105 , (e) 1.503 × 10–5 , (f) 6.07510 × 104arrow_forwardHow many significant figures are there in the following numbers? (a)0.00740 (b)609.20 (c)9.005 x 1011arrow_forwardCarry out the following conversions: (a) 1.42 lightyears to miles (a light-year is an astronomical measure of distance—the distance traveled by light in a year, or 365 days; the speed of light is 3.00x10^8 m/s), (b) 32.4 yd to centimeters, (c) 3.0 3x10^10 cm/s to ft/s.arrow_forward
- Perform the following calculations and report each answer with the correct number of significant figures.(a) 62.8 × 34(b) 0.147 + 0.0066 + 0.012(c) 38 × 95 × 1.792(d) 15 – 0.15 – 0.6155(e) 8.78 × ((0.0500)/(0.478))(f) 140 + 7.68 + 0.014(g) 28.7 – 0.0483(h) ((88.5 − 87.57)/(45.13))arrow_forwardLight travels in a vacuum at a speed of 3.00 × 108 m s-1 .(a) Convert this speed to miles per second.(b) Express this speed in furlongs per fortnight, a littleused unit of speed. (A furlong, a distance used in horse racing, is 660 ft; a fortnight is exactly 2 weeks.)arrow_forwardHow many significant figures are there in each of the following? (a) 61.8 ± 0.1 (b) 3.407 x 10⁹ (c) 2.0400 x 10-6 (d) 0.0040 Need Help? Read Itarrow_forward
- How many significant figures are there in each of the following?(a) 81.0 ± 0.8 (b) 3.827 ✕ 109 (c) 2.94 ✕ 10−6 (d) 0.0015arrow_forwardPerform the following arithmetic operations, and report the result to the proper number of significantfigures: (a) 1.0267 cm × 2.508 cm × 12.599 cm, (b) 15.0 kg ÷ 0.036 m3 , (c) 1.113 × 1010 kg − 1.050 × 109 kg, (d) 25.75 mL + 15.00 mL, (e) 46 cm3 + 180.5 cm3arrow_forwardA 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.arrow_forward
- The volume of a certain bacterial cell is 2.56 mm3. (a) What is its volume in cubic millimeters (mm3)? (b) What is the volume of 105 cells in liters (L)?arrow_forwardCalculate these masses.(a) What is the mass of 6.00 cm3 of mercury, density = 13.5939 g/cm3?(b) What is the mass of 25.0 mL octane, density = 0.702 g/cm3?arrow_forwardCalculate these masses.(a) What is the mass of 6.00 cm 3 of sodium, density = 0.97 g/cm 3 ?(b) What is the mass of 155 mL gaseous chlorine, density = 3.16 g/L?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning