Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
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Textbook Question
Chapter 10, Problem 97APP
When it rains or snows, the air temperature seems warmer. Explain. (10.7)
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1. (9 points) A 15.0 gram piece of metal is heated to 65.0°C and then dropped
into 175 grams of 24.0°C water. The system eventually comes to a stable
temperature of 35.5 C. (The specific heat of water is 4.184 J/g °C)
a. Energy is absorbed by the water. What is qWATER?
b. Energy is released by the metal. What is qMETAL? (this one is easy)
c. What is the specific heat (Cs) of the metal?
10.105 Complete and balance each of the following: (10.7)
a. ZnCO3(s) + H,SO,(aq)
b. Al(s) + HBr(aq)
Match each of the following
A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the
final temperature of water? ( specific heat of water = 4.18 J/g.°C ).
Choose...
Choose...
-48.25
188.7
A balloon of helium gas lost 36.4 kJ of heat while it was raising uP,
simultaneously, the helium gas expanded from 64.0 L to 80.0 L against 563
mmHg pressure, Calculate the change in the internal energy (AU) of helium gas (
in kJ). Given that (atm.L = 101.3 J)
-37.6
10.7
-238.7
39.0
268
11.85
Chapter 10 Solutions
Basic Chemistry
Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Prob. 3PPCh. 10.1 - If the available number of valence electrons for a...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.2 - Prob. 9PPCh. 10.2 - When does a molecular compound have resonance?
Ch. 10.2 - Draw two resonance structures for each of the...Ch. 10.2 - Draw two resonance structures for each of the...Ch. 10.3 - Prob. 13PPCh. 10.3 - Choose the shape (1 to 6) that matches each of the...Ch. 10.3 - Prob. 15PPCh. 10.3 - Prob. 16PPCh. 10.3 - Prob. 17PPCh. 10.3 - Prob. 18PPCh. 10.3 - Use VSEPR theory to predict the shape of each of...Ch. 10.3 - Prob. 20PPCh. 10.3 - Prob. 21PPCh. 10.3 - Draw the Lewis structure and predict the shape for...Ch. 10.4 - Describe the trend in electronegativity as...Ch. 10.4 - Describe the trend in electronegativity as...Ch. 10.4 - Prob. 25PPCh. 10.4 - Which electronegativity difference (a, b, or c)...Ch. 10.4 - Using the periodic table, arrange the atoms in...Ch. 10.4 - Using the periodic table, arrange the atoms in...Ch. 10.4 - Predict whether the bond between each of the...Ch. 10.4 - Predict whether the bond between each of the...Ch. 10.4 - For the bond between each of the following pairs...Ch. 10.4 - For the bond between each of the following pairs...Ch. 10.5 - Why is F2 a nonpolar molecule, but HF is a polar...Ch. 10.5 - Why is CCl4 a nonpolar molecule, but PCl3 is a...Ch. 10.5 - Identify each of the following molecules as polar...Ch. 10.5 - Identify each of the following molecules as polar...Ch. 10.5 - Prob. 37PPCh. 10.5 - Prob. 38PPCh. 10.6 - Prob. 39PPCh. 10.6 - Prob. 40PPCh. 10.6 - Identify the strongest intermolecular forces...Ch. 10.6 - Identify the strongest intermolecular forces...Ch. 10.6 - Prob. 43PPCh. 10.6 - Prob. 44PPCh. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Prob. 47PPCh. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Using Figure 10.6 and the specific heat of water,...Ch. 10.7 - Using Figure 10.6 and the specific heat of water,...Ch. 10.7 - An ice bag containing 275 g of ice at 0 °C was...Ch. 10.7 - Prob. 52PPCh. 10.7 - Prob. 53PPCh. 10.7 - In the preparation of liquid nitrogen, how many...Ch. 10.7 - Using the electronegativity values in Figure 10.2,...Ch. 10.7 - Prob. 56PPCh. 10.7 - Prob. 57PPCh. 10.7 - a. Draw two resonance structures for bicarbonate...Ch. 10 - State the number of valence electrons, bonding...Ch. 10 - State the number of valence electrons, bonding...Ch. 10 - Prob. 61UTCCh. 10 - Prob. 62UTCCh. 10 - Consider the following bonds: Ca and O, C and O, K...Ch. 10 - Consider the following bonds: F and Cl, Cl and Cl,...Ch. 10 - Identify the major intermolecular forces between...Ch. 10 - Prob. 66UTCCh. 10 - Prob. 67UTCCh. 10 - Prob. 68UTCCh. 10 - Prob. 69UTCCh. 10 - Prob. 70UTCCh. 10 - Prob. 71UTCCh. 10 - Prob. 72UTCCh. 10 - Prob. 73APPCh. 10 - Determine the total number of valence electrons in...Ch. 10 - Draw the Lewis structures for each of the...Ch. 10 - Draw the Lewis structures for each of the...Ch. 10 - Draw resonance structures for each of the...Ch. 10 - Prob. 78APPCh. 10 - Use the periodic table to arrange the following...Ch. 10 - Use the periodic table to arrange the following...Ch. 10 - Select the more polar bond in each of the...Ch. 10 - Select the more polar bond in each of the...Ch. 10 - Show the dipole arrow for each of the following...Ch. 10 - Show the dipole arrow for each of the following...Ch. 10 - Calculate the electronegativity difference and...Ch. 10 - Calculate the electronegativity difference and...Ch. 10 - Prob. 87APPCh. 10 - For each of the following, draw the Lewis...Ch. 10 - For each of the following, draw the Lewis...Ch. 10 - For each of the following, draw the Lewis...Ch. 10 - Prob. 91APPCh. 10 - Predict the shape and polarity of each of the...Ch. 10 - Prob. 93APPCh. 10 - Prob. 94APPCh. 10 - Prob. 95APPCh. 10 - Indicate the major type of intermolecular...Ch. 10 - When it rains or snows, the air temperature seems...Ch. 10 - Prob. 98APPCh. 10 - Using Figure 10.6, calculate the grams of ice that...Ch. 10 - Using Figure 10.6, calculate the grams of ethanol...Ch. 10 - Prob. 101APPCh. 10 - Using Figure 10.6, calculate the grams of benzene...Ch. 10 - Prob. 103CPCh. 10 - Prob. 104CPCh. 10 - Prob. 105CPCh. 10 - Prob. 106CPCh. 10 - Prob. 107CPCh. 10 - The melting point of benzene is 5.5 °C, and its...Ch. 10 - A 45.0-g piece of ice at 0.0 °C is added to a...Ch. 10 - An ice cube at 0 °C with a mass of 115 g is added...Ch. 10 - Prob. 111CPCh. 10 - Prob. 112CPCh. 10 - Prob. 13CICh. 10 - Prob. 14CICh. 10 - Prob. 15CICh. 10 - Ethanol, C2H6O , is obtained from renewable crops...Ch. 10 - Chloral hydrate, a sedative and hypnotic, was the...Ch. 10 - Ethylene glycol, C2H6O2 , used as a coolant and...Ch. 10 - Prob. 19CICh. 10 - Prob. 20CI
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- 28 A of ice at 0.0 °C is to a of at 8 A 45-g piece of ice at 0.0 °C is added to a sample of water at 8.0 °C. All of the ice melts and the temperature of the water decreases to 0.0 °C. How many grams of water were in the sample? (3.6, 3.7) oil in kcal/g? (3.5, 3.6) 9 In a large building, oil is used in a steam boiler heating system. The combustion of 1.0 lb of oil provides 2.4 × 107 J. (3.4, 3.6) a. How many kilograms of oil are needed to heat 150 kg of water from 22 °C to 100 °C? b. How many kilograms of oil are needed to change 150 kg of water to steam at 100 °C? 00 When 1.0 g of gasoline burns, it releases 11 kcal. The density of gasoline is 0.74 g/mL. (3.4, 3.6) a. How many megajoules are released when 1.0 gal of gaso- line burns? b. If a television requires 150 kJ/h to run, how many hours can the television run on the energy provided by 1.0 gal of gasoline? ISWERS wers to Selected Practice Problems a. element b. compound d. compound c. element e. compound a. pure substancearrow_forward(Q24) What is the density (in g/L) of sulfur dioxide gas at a pressure of 873 torr and a temperature of 69.0 °C? (3 sf)arrow_forward(Q21) A piston is filled with 2.13 mL of gas held at a pressure of 3.59 atm. What will the pressure (in atm) be if the piston expands to a volume of 7.45 mL? (3 sf)arrow_forward
- A quantity of 505 J of heat are added to 11.3 g of water at 28.3 0C. What is the final temperature of water? ( specific heat of water = 4.18 J/g.°C ). Choose... Choose... -37.6 39.0 268 A balloon of helium gas lost 36.4 kJ of heat while it was raising up, simultaneously, the helium gas expanded from 64.0 L to 80.0 L against 563 mmHg pressure. Calculate the change in the internal energy (AU) of helium gas ( in kJ) . Given that ( atm.L = 101.3 J) -238.7 -48.25 188.7 11.85 10.7 Thoose...arrow_forward16. A 200. g sample of titanium (specific heat of 0.52 J/g°C) is initially at 20.0 °C. If the sample absorbs 3600 J of heat, what is its final temperature? (2 points)arrow_forwardA quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the final temperature of water? ( specific heat of water = 4.18 J/g.0C ). Choose... Choose... -37.6 39.0 A balloon of helium gas lost 36.4 k) of heat while it was raising up, simultaneously, the helium gas expanded from 64.0L to 80.0 L against 563 mmHg pressure. Calculate the change in the internal energy (AU) of helium gas ( in kJ). Given that ( atm.L = 101.3 J) 268 -238.7 -48.25 188.7 11.85 10.7arrow_forward
- A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the final temperature of water? ( specific heat of water = 4.18 J/g.0C ). Choose... Choose... -37.6 39.0 268 A balloon of helium gas lost 36.4 kJ of heat while it was raising up, simultaneously, the helium gas expanded from 64.0 L to 80.0 L against 563 mmHg pressure. Calculate the change in the internal energy (AU) of helium gas ( in kJ). Given that ( atm.L = 101.3 J) -238.7 -48.25 188.7 11.85 10.7arrow_forwardA flask containing 1059 g of water is heated and a temperature increase from 32.4 °C to 67.6 °C. How much heat did one mole of water absorb in (J/mol). (s=4.18, molar mass of water 18 g/mol) a. 0.71 b. 4.30 C. 10.88 d. 2.50 е. 7.29 1.arrow_forward(Q4) A heated lead ball is added to 274 grams of water in a coffee cup calorimeter. If the ball loses 30.67 °C of heat and the water gains 2.9 °C of heat, what is the mass of the lead ball? (3 sf)arrow_forward
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