General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
5th Edition
ISBN: 9780321967466
Author: Karen C. Timberlake
Publisher: PEARSON
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Textbook Question
Chapter 3.7, Problem 3.51QAP
Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following:
- joules needed to melt 50.0 g of ice at 0 °C and to warm the liquid to 65.0 °C
- kilocalories released when 15.0 g of steam condenses at 100 °C and the liquid cools to 0 °C
- kilojoules needed to melt 24.0 g of ice at 0 °C, warm the liquid to 100 °C, and change it to steam at 100 °C
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Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following: a) joules needed to melt 50.0 g of ice at 0.00 deg C and to warm the liquid to 65.0\ deg C. b) kilocalories released when 15.0 g of steam condenses at 100. \deg C and the liquid cools to 0. \deg C.
Use the values for the heat of fusion, specific heat of water, and the heat of vaporization to calculate the total amount of heat in the following.
1. Joules released when 125 g of steam at 100 celsius condenses and cools to liquid at 15.0 Celcius.
2. Kilocalories needed to melt a 225 g ice sculpture at 0 celsius and to warm the liquid to 15 celsius.
A 149-g sample of steam at 100 ∘C is emitted from a volcano. It condenses, cools, and falls as snow at 0 ∘C. (For water, 80. cal (334 J) is needed to melt 1 gg of ice or must be removed to freeze 1 g of water and 540 cal (2260 J) is needed to convert 1 g of water to vapor at 100 ∘C.)
How many kilojoules of heat were released?
Chapter 3 Solutions
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Ch. 3.1 - Classify each of the following as a pure substance...Ch. 3.1 - Classify each of the following as a pure substance...Ch. 3.1 - Classify each of the following pure substances as...Ch. 3.1 - Classify each of the following pure substances as...Ch. 3.1 - 3.5 Classify each of the following mixtures as...Ch. 3.1 - Classify each of the following mixtures as...Ch. 3.2 - Indicate whether each of the following describes a...Ch. 3.2 - Indicate whether each of the following describes a...Ch. 3.2 - Prob. 3.9QAPCh. 3.2 - Describe each of the following as a physical or...
Ch. 3.2 - Prob. 3.11QAPCh. 3.2 - What type of change, physical or chemical, takes...Ch. 3.2 - Prob. 3.13QAPCh. 3.2 - Describe each property of the element zirconium as...Ch. 3.3 - Prob. 3.15QAPCh. 3.3 - Prob. 3.16QAPCh. 3.3 - Prob. 3.17QAPCh. 3.3 - Prob. 3.18QAPCh. 3.3 - Prob. 3.19QAPCh. 3.3 - Prob. 3.20QAPCh. 3.4 - Discuss the changes in the potential and kinetic...Ch. 3.4 - Prob. 3.22QAPCh. 3.4 - Prob. 3.23QAPCh. 3.4 - Prob. 3.24QAPCh. 3.4 - Prob. 3.25QAPCh. 3.4 - Prob. 3.26QAPCh. 3.5 - Calculate the kilocalories for each of the...Ch. 3.5 - Prob. 3.28QAPCh. 3.5 - Using the energy values for foods (see Table 3.7),...Ch. 3.5 - Prob. 3.30QAPCh. 3.5 - Prob. 3.31QAPCh. 3.5 - Prob. 3.32QAPCh. 3.5 - Prob. 3.33QAPCh. 3.5 - Prob. 3.34QAPCh. 3.6 - If the same amount of heat is supplied to samples...Ch. 3.6 - Prob. 3.36QAPCh. 3.6 - Prob. 3.37QAPCh. 3.6 - Use the heat equation to calculate the energy for...Ch. 3.6 - Use the heat equation to calculate the energy. in...Ch. 3.6 - Prob. 3.40QAPCh. 3.7 - Prob. 3.41QAPCh. 3.7 - Prob. 3.42QAPCh. 3.7 - Prob. 3.43QAPCh. 3.7 - Prob. 3.44QAPCh. 3.7 - Prob. 3.45QAPCh. 3.7 - Prob. 3.46QAPCh. 3.7 - Prob. 3.47QAPCh. 3.7 - Prob. 3.48QAPCh. 3.7 - Prob. 3.49QAPCh. 3.7 - Prob. 3.50QAPCh. 3.7 - Using the values for the heat of fusion, specific...Ch. 3.7 - Prob. 3.52QAPCh. 3.7 - Prob. 3.53QAPCh. 3.7 - Prob. 3.54QAPCh. 3.7 - Prob. 3.55QAPCh. 3.7 - Prob. 3.56QAPCh. 3 - Prob. 3.57UTCCh. 3 - Prob. 3.58UTCCh. 3 - Prob. 3.59UTCCh. 3 - Prob. 3.60UTCCh. 3 - Prob. 3.61UTCCh. 3 - Prob. 3.62UTCCh. 3 - Prob. 3.63UTCCh. 3 - Prob. 3.64UTCCh. 3 - Prob. 3.65UTCCh. 3 - Prob. 3.66UTCCh. 3 - Prob. 3.67UTCCh. 3 - Prob. 3.68UTCCh. 3 - Prob. 3.69AQAPCh. 3 - Prob. 3.70AQAPCh. 3 - Prob. 3.71AQAPCh. 3 - Prob. 3.72AQAPCh. 3 - Prob. 3.73AQAPCh. 3 - Prob. 3.74AQAPCh. 3 - Prob. 3.75AQAPCh. 3 - Prob. 3.76AQAPCh. 3 - Prob. 3.77AQAPCh. 3 - Prob. 3.78AQAPCh. 3 - Prob. 3.79AQAPCh. 3 - Prob. 3.80AQAPCh. 3 - Prob. 3.81AQAPCh. 3 - Prob. 3.82AQAPCh. 3 - 3.83 On a hot day, the bleach sand gets hot but...Ch. 3 - Prob. 3.84AQAPCh. 3 - Prob. 3.85AQAPCh. 3 - Prob. 3.86AQAPCh. 3 - Prob. 3.87AQAPCh. 3 - Prob. 3.88AQAPCh. 3 - Prob. 3.89AQAPCh. 3 - Prob. 3.90AQAPCh. 3 - If you want to lose 1 lb of “body fat,” which is...Ch. 3 - Prob. 3.92AQAPCh. 3 - Prob. 3.93AQAPCh. 3 - Prob. 3.94AQAPCh. 3 - Prob. 3.95CQCh. 3 - Prob. 3.96CQCh. 3 - Prob. 3.97CQCh. 3 - Prob. 3.98CQCh. 3 - Prob. 3.99CQCh. 3 - Prob. 3.100CQCh. 3 - Prob. 3.101CQCh. 3 - Prob. 3.102CQCh. 3 - Prob. 3.103CQCh. 3 - Prob. 3.104CQCh. 3 - Prob. 1CICh. 3 - Prob. 2CICh. 3 - Prob. 3CICh. 3 - Prob. 4CICh. 3 - Prob. 5CICh. 3 - Prob. 6CI
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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
- 1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)arrow_forwardOn a hot day, you take a six-pack ot a on a pcmc, cooling it with ice. Each empty (aluminum) can weighs 12.5 g. A can contains 12.0 oz of soda. The specific heat of aluminum is 0.902 J/g C; take that of soda to be 4.10 J/g C. (a) How much heat must be absorbed from the six-pack to lower the temperature from 25.00 to 5.00C? (b) How much ice must be melted to absorb this amount of heat? (Hfus of ice is given in Table 8.2.)arrow_forwardHow much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from 23.0 C to 1.0 C?arrow_forward
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