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chemistry principles and practice

Questions and Answers of Chemistry Principles And Practice

Identify the acid from its titration curve.The graphs shown in Exercises 16.90 through 16.93 are titration curves for 10.0 mL of 0.100 M acid with 0.100 M base. The identity of the acid is unknown,
Identify the acid from its titration curve.The graphs shown in Exercises 16.90 through 16.93 are titration curves for 10.0 mL of 0.100 M acid with 0.100 M base. The identity of the acid is unknown,
Identify the acid from its titration curve.The graphs shown in Exercises 16.90 through 16.93 are titration curves for 10.0 mL of 0.100 M acid with 0.100 M base. The identity of the acid is unknown,
Identify the acid from its titration curve.The graphs shown in Exercises 16.90 through 16.93 are titration curves for 10.0 mL of 0.100 M acid with 0.100 M base. The identity of the acid is unknown,
Calculate the volume of concentrated HCl (37% by weight, density 1.19 g/mL) that must be added to 500 mL of 0.10 M ammonia to make a buff er at pH 9.25.
What is the concentration of ammonium ion in a pH 9.00 solution that forms when concentrated NaOH is added to 0.100 M NH4Cl?
What is the pH of a solution that is saturated with iron(II) hydroxide?
A classical test for nitrogen in plant material involves adding some compounds to the plant material to produce ammonia (NH3, a base) from the nitrogen. The solution is then heated to drive off the
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a
A scientist has synthesized a diprotic organic acid, H2A, with a molar mass of 124.0 g/mol. The acid must be neutralized (forming the potassium salt) for an important experiment. Calculate the volume
Exactly 1.2451 g of a solid white acid is dissolved in water and completely neutralized by the addition of 36.69 mL of 0.404 M NaOH. Calculate the molar mass of the acid, assuming it to be a
What is a good indicator to use in the titration of a weak acid with Ka = 1.5 × 10-2?
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 83 mL of the concentrated HCl, adding it to water, and diluting to 1.00 L.(a)
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting
What is the work if a piston having an initial volume of 4.50 L expands to 7.65 L against a constant external pressure of 1.02 atm? Is work done on the system or by the system?StrategyFirst,
A cylinder contains 45.0 L of an ideal gas at a pressure of 140 atm . If the gas expands at a constant temperature against an opposing pressure of 0.970 atm , how much work (in joules) is done? The
A sample of gas in a balloon is compressed from 4.50 L to 1.00 L by an external pressure of 1.25 atm . At the same time, 60.0 J of heat is generated. Calculate ΔE.StrategyCalculate work using Pext
ΔE is -2.21 × 103 kJ/mol for the combustion of propane.Calculate ΔH for this reaction at 25 °C and 1.00 atm .StrategyUse Equations 17.3 and 17.4 to determine ΔH. The change in the number of
Determine the entropy change when 1 mol H2O boils at its normal boiling point of 100.0 °C . Th e heat of vaporization of water is 44.0 kJ/mol .StrategyWe will use Equation 17.5, remembering that
Calculate the standard entropy change when 1 mol of propane burns in oxygen.StrategyUse the standard molar entropies from Appendix G. For each product and reactant, do not forget to multiply the
Calculate ΔG° and determine whether the following reaction will take place spontaneously under standard-state conditions at 298 K.StrategyUse the standard Gibbs free energies of formation from
Consider the production of carbon dioxide and methane from carbon monoxide and hydrogen.StrategyUse Hess’s law to determine ΔH ° and ΔS °; then calculate ΔG °.
Calculate the Gibbs free-energy change for the reaction of nitrogen monoxide and bromine to form nitrosyl bromide at 298 K under two sets of conditions.(a) The partial pressure of each gas is 1.0 atm
The equilibrium constant for the following reaction is 1.0 × 1014 at 298 K .StrategyWe know that ΔG ° = -RT ln Keq, and we have values for Keq and T. Use the proper value and units for R so the
The standard Gibbs free-energy change for the following reaction is +55.69 kJ .StrategyBecause we know the ΔG ° and the temperature, we can use Equation 17.11 to determine the equilibrium
The vapor pressure of water at 25 °C is 23.77 torr , increasing to 42.20 torr at 35 °C . Calculate the standard free energy and standard enthalpy changes at 25 °C for the vaporization of
What is the work if a piston having an initial volume of 4.50 L contracts to 1.77 L against a constant external pressure of 1.34 atm? Is work done on the system or by the system?
Calculate the amount of work (in joules) done on the system when 6.30 × 103 L of an ideal gas (the system) initially at 1.00 atm is compressed at constant temperature and a pressure of 140 atm to a
A 7.56-g sample of gas is in a balloon that has a volume of 10.5 L. Under an external pressure of 1.05 atm, the balloon expands to a volume of 15.00 L. Then the gas is heated from 0.0 °C to 25.0
What is ΔH at 25 °C and 1.00 atm for the combustion of 1 mol ethane if ΔE = -1553 kJ?
Determine the entropy change when 1 mol H2O freezes at its normal freezing point of 0.0 °C. Th e heat of fusion of water is 6.01 kJ/mol.
Calculate the standard entropy change for the decomposition of hydrogen peroxide into water and oxygen. The reaction is:
Propene, C3H6, is proposed as a starting material in the production of butyraldehyde, C4H8O.
Calculate ΔG ° at 25 °C and at 300 °C for the synthesis of ammonia under standard conditions to determine whether the reaction is spontaneous at those temperatures.
Calculate the Gibbs free-energy change for the reaction of carbon dioxide and ammonia to form urea at 298 K, when all gases are present at 0.10-atm pressures.
The Keq for the formation of formaldehyde from water and carbon monoxide is 8.6 × 10-7.
The Gibbs free-energy change for the following reaction is +163.2 kJ.
The vapor pressure of methyl alcohol is 100 torr at 21.2 °C and 400 torr at 49.9 °C. What is the standard enthalpy of vaporization of methyl alcohol?
How is the sign of w, work, defined? How does it relate to the total energy of the system?
How is the sign of q, heat, defined? How does it relate to the total energy of the system?
Identify the sign of the work when a fuel-oxygen mixture (the system) burns, propelling an automobile (part of the surroundings).
What is the sign of the work when a refrigerator compresses a gas (the system) to a liquid during the refrigeration cycle?
When a rocket is launched, the burning gases are the source of the motion. If the system is the rocket (including fuel), what is the sign of the work?
A 125-L cylinder contains an ideal gas at a pressure of 100 atm. If the gas is allowed to expand against an opposing pressure of 0.0 atm at constant temperature, how much work (in kJ) is done?
State the first law of thermodynamics in words and in equation form. Define all symbols used in the equation.
State the conditions under which the heat absorbed by the system is equal to the change in enthalpy.
Explain the difference between internal energy and enthalpy.
Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined.
Explain why absolute entropies can be measured.
Under what conditions is the entropy of a substance equal to zero?
Explain why the entropy, S °, of an element in its standard state is not equal to zero despite the fact that ΔH°f and ΔG°f are equal to zero.
When most soluble ionic compounds dissolve in water, the enthalpy of solution is positive (the process is endothermic). What conclusion(s) can be made about the entropy change that accompanies the
A colleague states, “Since there is no detectable chemical change when methane (CH4) and oxygen mix, the reaction of these two substances is not spontaneous.” Explain what is wrong with this
When ice forms from liquid water at 0 °C and 1 atm pressure, ΔG is zero, because the change takes place under equilibrium conditions. Explain what the signs on the enthalpy change and entropy
Explain how the sign of the free energy as a criterion for spontaneity is a direct result of the second law of thermodynamics.
Give the relation between the change in free energy for a chemical reaction and the(a) Equilibrium constant.(b) Maximum useful work that can be obtained.(c) Free energy when reactants and products
The free energy for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either ΔH° or ΔS °.
Th e equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either ΔH° or ΔS °.
When solid sodium acetate crystallizes from a supersaturated solution, can you accurately predict the sign of ΔH for the crystallization? Why or why not?
When NaCl dissolves in water, can you accurately predict the sign of ΔH for the dissolution of the soluble salt? Why or why not?
What is the sign of w for the following processes if they occur at constant pressure? Consider only PV work from gases and assume that all gases behave ideally.
What is the sign of w for the following processes if they occur at constant pressure? Consider only PV work from gases, and assume that all gases behave ideally.
Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV work from the change in volume of gas, and assume that the gases are ideal and the chemical equation
Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV work from the change in volume of gas, and assume that the gases are ideal and the chemical equation
Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV work from the change in volume of gas, and assume that the gases are ideal and the chemical equation
Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV work from the change in volume of gas, and assume that the gases are ideal and the chemical equation
How much work is done if a balloon expands from 1.05 to 13.8 L against a constant external pressure of 1.08 atm?
Calculate the work performed if a balloon contracts from 12.90 L to 788 mL because of an external pressure of 3.70 atm.
A piston initially contains 0.400 L of air at 0.985 atm. What work is done if the piston contracts against a constant external pressure of 2.77 atm? The contraction will stop when the internal
A piston initially contains 688 mL of gas at 1.22 atm. What work is done if the piston expands against a constant external pressure of 733 torr? The expansion will stop when the internal pressure
A 220-L cylinder contains an ideal gas at a pressure of 150 atm. If the gas is allowed to expand against a constant opposing pressure of 1.0 atm, how much work is done? The expansion will stop when
A balloon contains 2.0 L helium at 1.10 atm. Calculate the work done if the gas expands against a constant atmospheric pressure of 754 torr. The expansion will stop when the internal pressure equals
For a process, w = -987 J and q = 555 J. What is ΔE for this process?
For a process, w = 34 J and q = -109 J. What is ΔE for this process?
Calculate w for a process in which q = 98 J and ΔE = 100 J.
Calculate q for a process in which w = 0 J and ΔE = 150 J.
A reaction between a solid and a liquid produces 4.5 L of a gas at 0.94 atm and absorbs 4.35 kJ of heat. Determine q, w, and ΔE for the reaction. (Assume an initial volume of 0.)
A reaction at 1.02 atm consumes 3.5 L of a gas and gives off 2.71 kJ of heat. Determine q, w, and ΔE for the reaction.
When an ideal gas expands at constant temperature (a condition referred to as isothermal ), ΔE is zero because the internal energy of an ideal gas depends only on temperature, not volume. Consider
When an ideal gas is compressed at constant temperature (isothermal conditions), ΔE is zero. Consider 9.00 L of a gas that is initially at 1.00 atm and 25 °C.(a) Calculate q and w if the gas sample
Explain why ΔH and ΔE are so similar in value for processes that do not involve gases.
Explain why ΔH and ΔE can be quite different in value for processes that involve gases.
The products of the combustion reaction of glycerin, C3H8O3, are gaseous carbon dioxide and liquid water.Write the balanced chemical equation for the combustion of 1 mol glycerin, and calculate ΔH
The products of the combustion reaction of n-propanol, C3H7OH, are gaseous carbon dioxide and liquid water. Determine the balanced chemical equation for the combustion of n-propanol, and calculate
Calculate ΔH°f for glycerin, C3H8O3, at 298 K using the H found in Exercise 17.45.Exercise 17.45The products of the combustion reaction of glycerin, C3H8O3, are gaseous carbon dioxide and liquid
Calculate ΔH°f for n-propanol, C3H7OH, at 298 K using the ΔH found in Exercise 17.46.Exercise 17.46The products of the combustion reaction of n-propanol, C3H7OH, are gaseous carbon dioxide and
What is the sign of the entropy change for each of the following processes? The system is underlined.(a) A plate is dropped on the floor and shatters.(b) A shuffled deck of cards is reordered from
Calculate the entropy change for the following processes.
Calculate the entropy change for the following processes.
Use data from Appendix G to calculate the standard entropy change for the following chemical reactions.
Use data from Appendix G to calculate the standard entropy change for the following chemical reactions.
Use the data in Appendix G to calculate the standard entropy change for
Use the data in Appendix G to calculate the standard entropy change for
Calculate ΔG ° for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K.
Calculate ΔG ° for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K.
Calculate ΔG ° for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K.
Calculate ΔG ° for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K.
Calculate ΔG for the following reactions two different ways:(1) use Hess’s law and the standard Gibbs free energies of formation, and(2) use ΔG = ΔH - TΔS. Compare the two values and judge
Calculate ΔG for the following reactions two diff erent ways:(1) Use Hess’s law and the standard Gibbs free energies of formation,(2) Use ΔG = ΔH - TΔS. Compare the two values and judge whether
Calculate ΔH °, ΔS °, and ΔG ° for each of the following reactions at 298 K. State whether the direction of spontaneous reaction is consistent with the sign of the enthalpy change, the entropy

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