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(a)
Interpretation:
Freezing water has to be classified as an endothermic or exothermic reaction.
Concept Introduction:
Exothermic reaction: Those reactions that release heat energy to the surroundings are called as exothermic reactions. The formation of
Endothermic reaction: Those reactions that absorb heat energy from the surroundings are called as endothermic reactions. The breakage of chemical bonds absorbs heat energy.
(b)
Interpretation:
The reaction inside an ice pack has to be classified as an endothermic or exothermic reaction.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Burning of wood has to be classified as an endothermic or exothermic reaction.
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
Combustion of magnesium in dry ice has to be classified as an endothermic or exothermic reaction.
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
Melting of ice has to be classified as an endothermic or exothermic reaction.
Concept Introduction:
Refer to part (a).
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Chapter 8 Solutions
FOUND.OF COLLEGE CHEMISTRY
- Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardHow is the addition of heat symbolized in a chemical equation? The addition of light energy?arrow_forward
- 4-21 The brilliant white light in some firework displays is produced by burning magnesium in air. The magne sium reacts with oxygen in the air to form magnesium oxide. Write a balanced equation for this reaction.arrow_forward4-77 To convert 1 mol of iron(III) oxide to its elements requires 196.5 kcal: How many grams of iron can be produced if 156.0 kcal of heat is absorbed by a large-enough sample of iron(III) oxide?arrow_forward4-25 In the chemical test for arsenic, the gas arsme, AsH3, is prepared. When arsine is decomposed by heating, arsenic metal deposits as a mirror-like coating on the surface of a glass container and hydrogen gas, H2, is given off. Write a balanced equation for the decomposition of arsine.arrow_forward
- 4.3 Explain the difference between complete and incomplete combustion.arrow_forward(a) Calcium and chlorine react to give calcium chloride in a combination reaction. Write and balance the equation. (b) Heating decomposes Na2CO3 to sodium oxide and carbon dioxide. Write and balance the equation.arrow_forwardAt 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction.arrow_forward
- Write a balanced equation describing each of the following chemical reactions.(a) Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas.(b) Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6.(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.arrow_forwardCombustion of hydrocarbons such as undecane (C11H24) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid undecane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.310kg of undecane are burned in air at a pressure of exactly 1atm and a temperature of 18.0°C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. = Larrow_forwardWhich observation is consistent with a chemical reaction occurring? Why?(a) Solid copper deposits on a piece of aluminum foil when the foil is placed in a blue copper nitrate solution. The blue color of the solution fades.(b) Liquid ethyl alcohol turns into a solid when placed in a low-temperature freezer.(c) A white precipitate forms when solutions of barium nitrate and sodium sulfate are mixed.(d) A mixture of sugar and water bubbles when yeasts are added. After several days, the sugar is gone and ethyl alcohol is found in the water.arrow_forward
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