Chemistry: Structure and Properties
1st Edition
ISBN: 9780321834683
Author: Nivaldo J. Tro
Publisher: PEARSON
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III. Perform these calculations and express the result with the proper number of
significant figures.
a. (4.850 g – 2.34 g)/1.3 mL
b. (4.66 x 10-3) × 4.666
c. 0.003400/65.2
Answer the following in the correct amount of significant figures
a. 4278 / 1.006=
b. 246.24 + 238.278+ 98.3=
c. 1.678 / 0.42=
d. (3.50 X 10^5) X [2.8 ÷ (5.4 ‐ 4.09)]=
a. Using the correct rules for multiplication/division and significant figures provide the answer for the following calculation.
6.98 x 89.44 =
b. Using the correct rules for multiplication/division and significant figures provide the answer for the following calculation.
7831 x 76.987 =
c. Using the correct rules for addition/subtraction and significant figures provide the answer for the following calculation.
7831 + 76.987 =
d. Using the correct rules for addition/subtraction and significant figures provide the answer for the following calculation.
7831.67 + 76.987 =
e. Using the correct rules for addition/subtraction and significant figures provide the answer for the following calculation.
7831.67 + 76.987 =
Chapter A2 Solutions
Chemistry: Structure and Properties
Ch. A2 - For each number, underline the zeroes that are...Ch. A2 - Prob. 2ECh. A2 - Prob. 3ECh. A2 - How many significant figures are in each number?...Ch. A2 - Prob. 5ECh. A2 - Indicate the number of significant figures in each...Ch. A2 - Round each number to four significant figures. a....Ch. A2 - Round each number to three significant figures. a....Ch. A2 - Prob. 9ECh. A2 - Prob. 10E
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- What is the difference between reporting the quantity nine inches as 9 inches and 9.00 inches?arrow_forward2. Do the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. a. 0.208 + 4.9 + 1.11 b. 228 + 0.999 + 1.02 c. 8.543 − 7.954 d.(3.2 × 10−2) + (5.5 × 10−1) (hint: Write in the decimal form first, then add.) e. 336.86 − 309.11 f. 21.66 − 0.02387arrow_forwardcalculate the following significant figures: a.) 7.890 x 1012/ 6.7 x 104 b.) (67.8 x 9.8)/ (100.04) c.)89.3 x 77.0 x 0.08arrow_forward
- Do the following multiplication and division calculations. Give a final answer with the correct number of significant figures and the correct units. Units can cancel or multiply just like number factors. (2.5 x 103 m/s) x (5.00 x 10-6 s) = ?arrow_forwardI keep getting this wrong and have gone over the problem 6 times and cant figure out what im doing wrong. I thought the answer was 3.125 Calculate 5.1234 + 0.033 ÷ 1.650 and report to the correct number of significant figures. a. 5.143 b. 3.125 c. 5.1 d. 3.1arrow_forwardpart A: Sort the following numbers according to whether they should be rounded up or down when rounding to the nearest tenth (the first digit after the decimal). 3.1760, 4.319, 19.47, 5.82, 66.9214, 8878.2010, 7.084, 124.76 part B: Drag the answers that have been correctly rounded to the appropriate number of significant figures to their place in the table. To avoid rounding errors, start with the unrounded value before conducting each manipulation. Drag the appropriate labels to their respective targets. View Available Hint(s)for Part B Reset Help 14.93 Group 3 14.93 12 Group 1 12 14.92 Group 3 14.92 3.62 Group 4 3.62 14 Group 3 14 3.7 Group 4 3.7 15 Group 3 15 3.6 Group 4 3.6 15.0 Group 3 15.0 3.63 Group 4 3.63 14.9 Group 3 14.9 3.623 Group 4 3.623 12.47 Group 1 12.47 7.97 Group 2 7.97 12.46 Group 1 12.46 7.966 Group 2 7.966 12.4 Group 1 12.4 7.0 Group 2 7.0 13 Group 1 13 7.96 Group 2 7.96 12.5 Group 1 12.5 8.0 Group 2 8.0 3.622 Group 1…arrow_forward
- Express each result to the proper number of significant figures 0.00071+0.002+0.00008 0.9827-0.06 14.9164-10.08+3282 8.13 x 102+8.13 x 103 1.784 x 104-3.6738 x 103 5.4989 x 10-3-1.5300 x 10-2arrow_forwardCalculate the correct number of significant figures. [(2.31*10^6) / 52.814] + 155.78=arrow_forward3. Perform the following calculations reporting your answer to the correct number of significant figures and with the correct units. a) 25.4 mL 21.4 mL = 1 1 kg b) 123.4 g * 1000 g c) 120.5 g + 32.567 g = conversion factors & calculations | EXP 2arrow_forward
- Express each result to the proper number of significant figures 5698 x 0.0439 0.005493/(28.000 x 10-1) 3.14 x 22.00 x 166/12 (45.0 x 102)2 (35.67 x 10-5)1/3 (44.963-44.960) x 7.3182 82.32-79.4/365.99arrow_forwardQ.1. A student obtains the number 0.40076 on a balance. 4.00 x10 If this number actually has (3) significant figures, how should it be written? 0.400 0.4007 0.401 Q.2. Convert 5324 mL to m' (1000 L=1 m') 5.324 x10 5.324 5.324x10' 0.5324x10 Q.3. A student wants 25.0 g of acetone for a chemical 31.605 mL reaction. If the density of acetone is 0.791 g/mL, how many milliliters of acetone are needed? (take care about significant figures) 0.316 x10 19.7 19.77 Multiple optionalarrow_forwardI. Significant Figures and Conversion A. Scientific Notation 1. 58 cm → km 2. 67 W → MW 3. 196 mL L 4. 17 dm – cm 5. 299 W → TWarrow_forward
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