Principles of General, Organic, Biological Chemistry
2nd Edition
ISBN: 9780073511191
Author: Janice Gorzynski Smith Dr.
Publisher: McGraw-Hill Education
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Chapter 4.6, Problem 4.20P
(a)
Interpretation Introduction
Interpretation:
The energy in calories when
(b)
Interpretation Introduction
Interpretation:
The energy in calories when
(c)
Interpretation Introduction
Interpretation:
The energy in kilocalories when
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Students have asked these similar questions
Identify the property of water that explains why these phenomena happen. 1. The water in swimming pool remains cool even in summer. 2.Ice floats in a glass of water.3. The evaporation of sweat, cools the body to maintain a steady temperature.
4. Beading of water on a waxed car.5. Bubbles of vapor form within the liquid and rise to the surface.
Which statement below would be accurate about freezing water (AH°fus
for water 40.7 kJ/mol) ?
O Freezing water is an exothermic process and to form the intermolecular forces
that hold together the water molecules absorbing 40.7 kJ/mol of energy.
O Freezing water is an exothermic process and to form the intermolecular forces
that hold together the water molecules releasing 40.7 kJ/mol of energy.
O Freezing water is an endothermic process and to form the intermolecular
forces that hold together the water molecules releasing 40.7 kJ/mol of energy.
When 4.61 grams of ice at - 20°C have
absorbed 2500 calories of heat, what is the
temperature of the resulting water?
specific heat of ice = 0.50 cal/g°c
specific heat of water = 1.0 cal/g °C
latent heat of fusion = 80 cal /g
Chapter 4 Solutions
Principles of General, Organic, Biological Chemistry
Ch. 4.1 - Prob. 4.1PCh. 4.1 - Prob. 4.2PCh. 4.1 - Prob. 4.3PCh. 4.1 - Prob. 4.4PCh. 4.2 - Prob. 4.5PCh. 4.2 - Prob. 4.6PCh. 4.3 - Prob. 4.7PCh. 4.3 - Prob. 4.8PCh. 4.3 - Prob. 4.9PCh. 4.3 - Prob. 4.10P
Ch. 4.3 - Which of the compounds in each pair has stronger...Ch. 4.4 - Prob. 4.12PCh. 4.4 - Prob. 4.13PCh. 4.5 - A student has two containers one with 10 g of...Ch. 4.5 - Prob. 4.15PCh. 4.5 - How much energy is required to heat 28.0 g of iron...Ch. 4.5 - Prob. 4.17PCh. 4.5 - Prob. 4.18PCh. 4.5 - Prob. 4.19PCh. 4.6 - Prob. 4.20PCh. 4.6 - Prob. 4.21PCh. 4.6 - Label each process as endothermic or exothermic...Ch. 4.6 - Prob. 4.23PCh. 4.7 - Answer the following questions about the graph. a....Ch. 4.7 - Prob. 4.25PCh. 4.7 - If the cooling curve in Figure 4.5 represented a...Ch. 4.7 - How much energy (in calories) is released when...Ch. 4.7 - Prob. 4.28PCh. 4 - What phase change is shown in the accompanying...Ch. 4 - What phase change is shown in the accompanying...Ch. 4 - Consider the cooling curve drawn below. a. Which...Ch. 4 - Which line segments on the cooling curve in...Ch. 4 - Prob. 4.33UKCCh. 4 - Prob. 4.34UKCCh. 4 - Prob. 4.35UKCCh. 4 - Prob. 4.36UKCCh. 4 - Prob. 4.37UKCCh. 4 - Prob. 4.38UKCCh. 4 - Prob. 4.39APCh. 4 - Prob. 4.40APCh. 4 - Prob. 4.41APCh. 4 - Prob. 4.49APCh. 4 - Prob. 4.50APCh. 4 - Prob. 4.54APCh. 4 - Prob. 4.55APCh. 4 - Prob. 4.56APCh. 4 - Prob. 4.57APCh. 4 - Prob. 4.58APCh. 4 - Prob. 4.59APCh. 4 - Prob. 4.60APCh. 4 - Prob. 4.61APCh. 4 - Prob. 4.62APCh. 4 - Prob. 4.63APCh. 4 - Prob. 4.64APCh. 4 - Prob. 4.65APCh. 4 - Prob. 4.66APCh. 4 - Prob. 4.67APCh. 4 - Prob. 4.68APCh. 4 - Prob. 4.69APCh. 4 - Prob. 4.70APCh. 4 - Prob. 4.71APCh. 4 - Prob. 4.72APCh. 4 - Prob. 4.73APCh. 4 - Prob. 4.74APCh. 4 - Prob. 4.75APCh. 4 - Prob. 4.76APCh. 4 - Prob. 4.77APCh. 4 - Prob. 4.78APCh. 4 - Prob. 4.79APCh. 4 - Why does steam form when hot lava falls into the...Ch. 4 - Prob. 4.81APCh. 4 - Prob. 4.82AP
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- A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).arrow_forwardSubstance A is composed of molecules that have stronger intermolecular forces than the molecules that compose substance B. Which substance has a lower boiling point? a. substance A b. substance B c. cannot be determined without more information.arrow_forwardUse the heating-cooling curve below to answer the following questions. a. What is the freezing point of the liquid? b. What is the boiling point of the liquid? c. Which is greater, the heat of fusion or the heat of vaporization? Explain each term and explain how the heating-cooling curve above helps you to answer the question.arrow_forward
- What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.arrow_forwardExplain why evaporation leads to cooling of the liquid.arrow_forwardConsider a substance X with a Hvap = 20.3 kJ/mol and Hfus = 9.0 kJ/mol. The melting point, freezing point, and heat capacities of both the solid and liquid X are identical to those of water. a If you place one beaker containing 50 g of X at 10C and another beaker with 50 g of H2O at 10C on a hot plate and start heating them, which material will reach the boiling point first? b Which of the materials from part a, X or H2O, would completely boil away first? c On a piece of graph paper, draw the heating curve for H2O and X. How do the heating curves reflect your answers from parts a and b?arrow_forward
- Is it possible to liquefy nitrogen at room temperature (about 25 C)? Is it possible to liquefy sulfur dioxide at room temperature? Explain your answers.arrow_forwardThe graph below represents the heating curve of a substance that starts as a solid below its freezing point. 120- 90 60 30 Time (minutes) What is the melting point of this substance? Which letter represents the state with no intermolecular force? Which letter represents the process Melting? Which letter represents the state where molecules move slowly? Temperature (C)arrow_forwardCalculate the heat change in calories for melting of 0.30 kg of water at 0*C. The heat of fusion for water is 80 cal/g. The heat of vaporization of water is 540 cal/g. The specific heat capacity of water is 1.00 cal/J*C.arrow_forward
- compound y has a heat of fusion of 363 J/g the solid form has a specific heat capacity of 0.238 J/g°C and the liquid form has a specific heat capacity of 2.68 J/g°C the freezing point of compound y is -13.8°C. how much energy will it take to convert a 303.8 g solid sample of y at -29.7°C to a sample at 42.1°C? give answer in kJ make sure it is rounded to the correct number of sig figsarrow_forwardWhich statement below would be accurate about boiling water? Boiling water is an exothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules release 40.7 kJ of energy. Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.arrow_forwardHow toarrow_forward
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