1. 27 JJ to calories Express your answer using two significant figures. 2. 5300 JJ to kilojoules Express your answer using two significant figures. 3. 374 kJkJ to joules Express your answer using three significant figures.
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- Determine the amount of potassium chloride in each solution. 18.9 g of a solution containing 1.12 % KCl by mass Express your answer in grams using three significant figures. 29.2 kg of a solution containing 20.7 % KCl by mass Express your answer in kilograms using three significant figures. 45 mg of a solution containing 14 % KCl by mass Express your answer in milligrams using two significant figures.Perform each conversion between energy units. 3.71×106 kJ to kcal Express the value in kilocalories to three significant figures.To how many significant figures should each answer be rounded? (6.626x 10-34 J . s) (2.9979x 10% m/s) equation A: = 4.483992189616 x 10-19 J (unrounded) 4.430 x 10-7 m After rounding, the answer to equation A should have O 1 significant figure. O 4 significant figures. O 2 significant figures. O 3 significant figures. O 5 significant figures. (6.022x 1023 atoms/mol) (0.653 g) 20.18 g/mol = 1.949 x 1022 atoms (unrounded) equation B: After rounding, the answer to equation B should have
- © 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. K1. It is known that the boiling point of water on the Kelvin temperature scale is 373.15 K and the freezing temperature of water is 273.15 K. A temperature scale, called the Reaumur (R) scale, is defined by identifying the freezing point of water as 0.0°R and the boiling point of water as 80.0°R. What is 62.3°R on the Kelvin scale? Clearly define your variables.The specific heat of copper metal is 0.385 J/g.°C. How many joules of heat are required to raise the temperature of a 2.80 kg block of copper from 25.0°C to 91.0 °C? Report your answer with the correct number of significant figures in regular form. Do not include units in your answer.
- Mass of cup + water Mass of empty cup Mass of water Initial water temperature Final water temperature Change in water temperature 103.4 g 1.6 g ? A 8400 Joules B 101.6 Joules C 3300 Joules D 7.80 Joules 19.8°C 27.6°C ? 15. For the laboratory data above, determine the amount of energy absorbed/lost by the water in joules. Round your answer to the correct number of significant figures. (Specific Heat of water= 4.18 J/g °C)To how many significant figures should each answer be rounded? equation A: (6.626× 10−34 J⋅s)(2.9979× 108 m/s)4.650×10−7 m=4.271846322581×10−19 J(unrounded) After rounding, the answer to equation A should have 1 significant figure. 2 significant figures. 3 significant figures. 5 significant figures. 4 significant figures. equation B: (6.022× 1023 atoms/mol)(0.787 g)20.18 g/mol=2.349×1022 atoms(unrounded) After rounding, the answer to equation B should have 2 significant figures. 3 significant figures. 5 significant figures. 4 significant figures. 1 significant figure.A single 1−oz serving of tortilla chips contains 260 mg of sodium. If an individual ate the entire 18−oz bag, how many grams of sodium would he ingest? If the recommended daily intake of sodium is 2.4 g, does this provide more or less than the recommended daily value, and by how much?He would ingest ____g of sodium. Thus, the entire bag of chips provides more than the recommended daily allowance of sodium by ____g.
- To how many significant figures should each answer be rounded? equation A: (6.626× 10−34 J⋅s)(2.9979× 108 m/s)4.610×10−7 m=4.308912234273×10−19 J(unrounded) After rounding, the answer to equation A should have 5 significant figures. 3 significant figures. 4 significant figures. 1 significant figure. 2 significant figures. equation B: (6.022× 1023 atoms/mol)(0.469 g)20.18 g/mol=1.400×1022 atoms(unrounded) After rounding, the answer to equation B should have 1 significant figure. 2 significant figures. 3 significant figures. 4 significant figures. 5 significant figures.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…One student calibrated a 50-mL burette by using the mass of water delivered. The student used an analytical balance which was previously calibratedby STEEL (density = 7.8 g/mL). During calibration, the temperature of water was found to be 19.0oC. The density of water at this temperature is0.9984 g/mL. The results of the calibration by the student is shown in the table below:A B C D EApparent burette reading, mL 10.05 20.04 30.08 40.07 49.98Weight H2O delivered, g 10.03 20.09 30.05 40.02 49.83Note: All masses in mentioned in this section are understood to be in grams and all volumes mentioned are understood to be in milliliters. What is the true volume of water delivered in D?A) 40.11B) 40.12C) 40.13D) 40.14E) 40.15
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