The complete combustion of ethanol, C₂H₅OH(l), to form H₂O(g) and CO₂(g) at constant pressure releases 1235 kJ of heat per mole of C₂H₅OH. b. Draw an enthalpy diagram for the reaction.

The decomposition of Ca(OH)₂ into CaO(s) and H₂O at constant pressure requires the addition of 109 kJ of heat per mole of Ca(OH)₂ . b. Draw an enthalpy diagram for the reaction.

Ozone, O₃(g), is a form of elemental oxygen that plays an important role in the absorption of ultraviolet radiation in the stratosphere. It decomposes to O₂(g) at room temperature and pressure according to the following reaction: 2 O₃(g) → 3 O₂(g) ΔH= -284.6 kJ b. Which has the higher enthalpy under these conditions, 2 O₃(g) or 3 O₂(g)?

Without referring to tables, predict which of the following has the higher enthalpy in each case: (a) 1 mol CO₂(s) or 1 mol CO₂(g) at the same temperature

Without referring to tables, predict which of the following has the higher enthalpy in each case: (b) 2 mol of hydrogen atoms or 1 mol of H₂

Without referring to tables, predict which of the following has the higher enthalpy in each case: (c) 1 mol H₂(g) and 0.5 mol O₂(g) at 25 °C or 1 mol H₂O(g) at 25 °C

Consider the following reaction: 2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252.8 kJ (b) Calculate the amount of heat transferred when 24.0 g of CH₃OH(g) is decomposed by this reaction at constant pressure.

Consider the following reaction: 2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252.8 kJ (d) How many kilojoules of heat are released when 38.5 g of CH₄(g) reacts completely with O₂(g) to form CH₃OH(g) at constant pressure?

When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates Ag⁺(aq) + Cl^-(aq) → AgCl(s) H = -65.5 kJ (a) Calculate H for the production of 0.450 mol of AgCl by this reaction. (b) Calculate H for the production of 9.00 g of AgCl. (c) Calculate H when 9.25⨉10^-4 mol of AgCl dissolves in water.

At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO₃: 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) ΔH = -89.4 kJ For this reaction, calculate H for the formation of (a) 1.36 mol of O₂

At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO₃: 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) ΔH = -89.4 kJ For this reaction, calculate H for the formation of (b) 10.4 g of KCl.

At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO₃: 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) ΔH = -89.4 kJ c. Now consider the reverse reaction, in which KClO₃ is formed from KCl and O₂. What is Δ𝐻 for the formation of 19.1 g KClO₃ from KCl and O₂?

Consider the combustion of isopropanol, C₃H₇OH(l), which is the primary component of rubbing alcohol: C₃H₇OH(l) + 9/2 O₂(g) → 3 CO₂(g) + 4 H₂O(l) ΔH = -2248 kJ a. What is the enthalpy change for the reverse reaction?

Consider the combustion of isopropanol, C₃H₇OH(l), which is the primary component of rubbing alcohol: C₃H₇OH(l) + 9/2 O₂(g) → 3 CO₂(g) + 4 H₂O(l) ΔH = -2248 kJ (b) Balance the forward reaction with whole-number coefficients. What is ΔH for the reaction represented by this equation?

Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g): C₆H₆(l) → 3 C2H₂(g) ΔH = +630 kJ (a) What is the enthalpy change for the reverse reaction?

Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g): C₆H₆(l) → 3 C2H₂(g) ΔH = +630 kJ (b) What is H for the formation of 1 mol of acetylene?

Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g): C₆H₆(l) → 3 C2H₂(g) ΔH = +630 kJ (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction?

Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g): C₆H₆(l) → 3 C2H₂(g) ΔH = +630 kJ (d) If C₆H₆(g) were consumed instead of C₆H₆(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.

b. What are the units of specific heat?

Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g of water at 10.0 °C. Object A increases the water temperature by 3.50 °C; B increases the water temperature by 2.60 °C. (a) Which object has the larger heat capacity?

(c) What is the heat capacity of 185 g of liquid water?

(d) How many kJ of heat are needed to raise the temperature of 10.00 kg of liquid water from 24.6 to 46.2 °C?

(b) Calculate the energy needed for this temperature change.

The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. (a) How many J of heat are needed to raise the temperature of 80.0 g of octane from 10.0 to 25.0 °C?

The specific heat of ethanol, C₂H₅OH(l), is 2.44 J•g/K. b. Which will require more heat, increasing the temperature of 1 mol of C₂H₅OH(𝑙) by a certain amount or increasing the temperature of 1 mol of H₂O(𝑙) by the same amount?

Consider the data about gold metal in Exercise 5.24(b). b. Suppose that the same amount of heat is added to two 10.0-g blocks of metal, both initially at the same temperature. One block is gold metal, and the other is iron metal. Which block will have the greater rise in temperature after addition of the heat?

Consider the data about gold metal in Exercise 5.24(b). c. What is the molar heat capacity of Au(s)?

When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. a. Calculate the quantity of heat (in kJ) released in the reaction.

When a 5.10-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 20.5 to 33.2 °C. b. Using your result from part (a), calculate ΔH (in kJ/mol NaOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.