All Matches

Solution Library

Expert Answer

Textbooks

Search Textbook questions, tutors and Books

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Tutors
Study Help
Ask a Question

Search
Sign In
Register

study help
sciences
chemical principles

Questions and Answers of Chemical Principles

Calculate(a) The molality of chloride ions in an aqueous solution of iron(III) chloride for which xFeCl3 = 0.0312;(b) The molality of hydroxide ions in a solution prepared from 3.24 g of barium
Analysis of a reaction mixture showed that it had the composition 0.520 mol · L–1 N2, 0.485 mol · L–1 H2, and 0.102 mol · L–1 NH3 at 800. K, at which temperature Kc = 0.278 for N2(g) + 3
Explain what happens to the solubility of the CO2 in Exercise 5D.9 if(a) The partial pressure of CO2(g) is increased by compressing the gas to a third of its original volume;(b) The temperature is
The vapor pressure of chlorine dioxide, ClO2, is 155 Torr at 222.75 °C and 485 Torr at 0.00 °C. Calculate(a) The standard enthalpy of vaporization;(b) The standard entropy of
A sample of a polypeptide of mass 0.40 g dissolved in 1.0 L of an aqueous solution at 27 8C gave rise to an osmotic pressure of 3.74 Torr. What is the molar mass of the polypeptide?
The height of a column of liquid that can be supported by a given pressure is inversely proportional to its density. An aqueous solution of 0.010 g of a protein in 10. mL of water at 20°C shows a
Benzene, C6H6, and toluene, C6H5CH3, form an ideal solution. The vapor pressure of benzene is 94.6 Torr and that of toluene is 29.1 Torr at 25°C. Calculate the total vapor pressure of each of the
Write the reaction quotient Q for (a) 2 BCl3(g) + 2 Hg(1)→ B₂Cl(s) + Hg₂Cl₂(s) (b) P4S10(s) + 16 H₂O(1)→ 4 H3PO4(aq) + 10 H₂S(aq) (c) Br₂(g) + 3 F₂(g) →2 BrF3(g)
Predict whether each of the following equilibria will shift toward products or reactants with a temperature increase: 2 NO₂(g), AH° = +57 kJ 2 X(g), where X is a halogen → (a) N₂O4(g) (b)
(a) Calculate the mass of CaCl2 · 6H2O needed to prepare 0.125 m CaCl2(aq) by using 500. g of water.(b) What mass of NiSO4 · 6H2O must be dissolved in 500. g of water to produce 0.22 m NiSO4(aq)?
A soft drink is made by dissolving CO2 gas at 3.60 atm in a flavored solution and sealing the solution in aluminum cans at 20°C. What amount (in moles) of CO2 is contained in a can of the soft drink
A reaction vessel of volume 0.500 L at 700. K contains 1.20 mmol SO2(g), 0.50 mmol O2(g), and 0.10 mmol SO3(g). At 700. K, Kc = 1.7 * 106 for the equilibrium 2 SO2(g) + O2(g) ⇌ 2 SO3(g). (a)
The normal boiling point of iodomethane, CH3I, is 42.43°C, and its vapor pressure at 0.00°C is 140. Torr. Calculate(a) The standard enthalpy of vaporization of iodomethane;(b) The standard
A solution prepared by adding 0.50 g of a polymer to 0.200 L of toluene (methylbenzene, a common solvent) showed an osmotic pressure of 0.582 Torr at 20 8C. What is the molar mass of the polymer?
Predict whether each of the following equilibria will shift toward products or reactants with a temperature increase: (a) CH4(g) + H₂O(g) (b) CO(g) + H₂O(g) (c) 2 SO₂(g) + O₂(g) CO(g) +3
Hexane, C6H14, and cyclohexane, C6H12, form an ideal solution. The vapor pressure of hexane is 151 Torr and that of cyclohexane is 98 Torr at 25.0°C. Calculate the total vapor pressure of each of
A 0.060 m C6H12O6(aq) solution (glucose) is separated from a 0.040 m CO(NH2)2(aq) solution (urea) by a semipermeable membrane at 25°C. For both compounds, i = 1. (a) Which solution has the higher
The density of a 10.0% by mass H2SO4(aq) solution is 1.07 g · cm–3.(a) What volume (in milliliters) of solution contains 8.37 g of H2SO4?(b) What is the molality of H2SO4 in the
A soft drink is made by dissolving CO2 gas at 4.00 atm in a flavored solution and sealing the solution in aluminum cans at 20°C. What amount (in moles) of CO2 is contained in a can of the soft drink
Given that Kc = 62 for the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) at 500. K, calculate whether more ammonia will tend to form when a mixture of composition 1.25 mmol · L–1 N2, 4.58 mmol · L–1
The normal boiling point of ethyl acetate, CH3COOC2H5, used to remove nail polish, is 77.1°C, and its vapor pressure at 16.2 °C is 10.0 kPa. Calculate(a) The standard enthalpy of vaporization of
(a) From data in Appendix 2A, derive a numerical form of the Clausius–Clapeyron equation for methanol.(b) Use the equation to plot the appropriate quantities that should give a straightline
A polymer sample of mass 0.20 g dissolved in 0.100 L of toluene, gives rise to an osmotic pressure of 6.3 Torr at 20°C.What is the molar mass of the polymer?
The vapor pressure of 1,1-dichloroethane, CH3CHCl2, is 228 Torr at 25°C; at the same temperature, that of 1,1-dichlorotetrafluoroethane, CF3CCl2F, is 79 Torr. What mass of 1,1-dichloroethane must be
(a) Calculate the reaction Gibbs free energy of I2 (g) → 2 I (g) at 1200. K (K = 6.8) when the partial pressures of I2 and I are 0.13 bar and 0.98 bar, respectively.(b) Indicate whether this
A gaseous mixture consisting of 2.23 mmol N2 and 6.69 mmol H2 in a 500.-mL container was heated to 600. K and allowed to reach equilibrium. Will more ammonia be formed if that equilibrium mixture is
(a) From data in Appendix 2A and Table 4C.1, derive a numerical form of the Clausius–Clapeyron equation for benzene.(b) Use the equation to plot the appropriate quantities that should give a
Lithium sulfate dissolves exothermically in water.(a) Is the enthalpy of solution for Li2SO4 positive or negative?(b) Write the chemical equation for the dissolving process.(c) Which is larger for
(a) In an experiment, 2.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L and heated to 1000. K to study its dissociation into Cl atoms. Use the information in Table 5G.2 to calculate
Catalase, a liver enzyme, dissolves in water. A solution of volume 10.0 mL containing 0.166 g of catalase gives rise to an osmotic pressure of 1.2 Torr at 20°C. What is the molar mass of catalase?
The vapor pressure of butanone, CH3CH2COCH3, is 100. Torr at 25°C; at the same temperature that of propanone, CH3COCH3, is 222 Torr. What mass of propanone must be mixed with 350.0 g of butanone to
Calculate the reaction Gibbs free energy of PCl3(g) 1 Cl2(g) → PCl5(g) at 230 8C when the partial pressures of PCl3, Cl2, and PCl5 are 0.35 bar, 0.45 bar, and 1.02 bar, respectively. What is the
A gaseous mixture consisting of 1.1 mmol SO2 and 2.2 mmol O2 in a 250-mL container was heated to 500. K and allowed to reach equilibrium. Will more sulfur trioxide be formed if that equilibrium
The enthalpy of solution of ammonium nitrate in water is positive.(a) Does NH4NO3 dissolve endothermically or exothermically?(b) Write the chemical equation for the dissolving process.(c) Which is
Calculate the osmotic pressure at 20°C of each of the following solutions, assuming complete dissociation for any ionic solutes:(a) 0.050 m C12H22O11(aq);(b) 0.0010 m NaCl(aq);(c) A saturated
Calculate the equilibrium constant at 25°C and at 150°C for each of the following reactions, using data available in Appendix 2A: (a) NH4Cl(s) (b) H₂(g) + D₂O(1) NH3(g) + HCl (g) D₂(g) +
Which of the following mixtures would you expect to show a positive deviation, a negative deviation, or no deviation (that is, form an ideal solution) from Raoult’s law? Explain your
Colligative properties can be sources of insight into not only the properties of solutions, but also the properties of the solute. For example, acetic acid, CH3COOH, behaves differently in two
Calculate the heat evolved or absorbed when 10.0 g of(a) NaCl;(b) NaI;(c) AlCl3;(d) NH4NO3 is dissolved in 100. g of water. Assume that the enthalpies of solution in Table 5D.3 are applicable and
(a) Calculate the reaction Gibbs free energy of N2(g)+ 3 H2(g) → 2 NH3(g) when the partial pressures of N2, H2, and NH3 are 4.2 bar, 1.8 bar, and 21 bar, respectively, and the temperature is
When solid NH4HS and 0.400 mol NH3 (g) were placed in a vessel of volume 2.0 L at 24°C, the equilibrium NH4HS(s) ⇌ NH3 (g) + H2S(g), for which Kc = 1.6 * 10–4, was reached. What are the
Calculate the equilibrium constant at 25°C and at 100°C for each of the following reactions, using data available in Appendix 2A: (a) 2 CuO (s) 2 Cu(s) + O(g) (b) CH4(g) + H(g) CH6(g)
Determine the temperature change when 4.00 g of(a) KCl;(b) MgBr2;(c) KNO3;(d) NaOH is dissolved in 100. g of water.Assume that the specific heat capacity of the solution is 4.18 J · K–1 ·
Calculate the osmotic pressure at 20°C of each of the following solutions, assuming complete dissociation of ionic compounds:(a) 4.5 * 10–3 m C6H12O6(aq);(b) 3.0 * 10–3 m CaCl2(aq);(c) 0.025
Which of the following mixtures would you expect to show a positive deviation, a negative deviation, or no deviation (that is, form an ideal solution) from Raoult’s law? Explain your
Standard practice in chemical laboratories is to distill highboiling-point substances under reduced pressure. Trichloroacetic acid has a standard enthalpy of vaporization of 57.8 kJ · mol–1 and a
(a) Calculate the reaction Gibbs free energy of H2(g) 1 I2(g) → 2 HI(g) at 700. K when the partial pressures of H2, I2, and HI are 0.35 bar, 0.18 bar, and 2.85 bar, respectively. For this
(a) When solid NaHCO3 was placed in a rigid container of volume 2.50 L and heated to 160.°C, the equilibrium 2 NaHCO3(s) ⇌ Na2CO3(s) + CO2(g) + H2O(g) was reached. At equilibrium, some of the
The temperature-dependence of the vapor pressure of phosphoryl chloride difluoride (OPClF2) has been measured:(a) Plot ln P against 1/T (this plot is best created with the aid of a computer or a
Depict the progress of the reaction graphically (as in Fig. 5G.1) for the reaction in Exercise 5G.13.Exercise 5G.13(a) Calculate the reaction Gibbs free energy of I2 (g) → 2 I (g) at 1200. K (K =
By combining the relation for Kc in terms of K with the van ’t Hoff equation, find the analog of the van ’t Hoff equation for Kc.
Distinguish between a foam and a sol. Give at least one example of each.
The equilibrium constant Kc for the reaction N2(g) + O2(g) ⇌ 2 NO(g) at 1200°C is 1.00 * 10–5. Calculate the equilibrium molar concentrations of NO, N2, and O2 in a reaction vessel of volume
From literature sources, find the critical pressures and temperatures of methane, methylamine (CH3NH2), ammonia, and tetrafluoromethane. Discuss the suitability of using each of these solvents for a
Depict the progress of the reaction graphically (as in Fig. 5G.1) for the reaction in Exercise 5G.13 if the starting partial pressures of I2 and I are 0.75 bar and 0.12 bar, respectively.Exercise
The vaporization of a liquid can be treated as a special case of an equilibrium. How does the vapor pressure of a liquid vary with temperature? Devise a version of the van ’t Hoff equation that
Distinguish between an emulsion and a gel. Give at least one example of each.
Calculate the standard Gibbs free energy of each of the following reactions: (a) I₂(g) 2 I(g), K = 6.8 at 1200. K (b) Ag₂ CrO4(s) = 2 Ag+ (aq) + CrO₂²(aq), K 1.1 X 10-12 at 298 K
The equilibrium constant Kc for the reaction N2(g) + O2 (g) ⇌ 2 NO(g) at 1200°C is 1.00 * 10–5. Calculate the equilibrium molar concentrations of NO, N2, and O2 in a reaction vessel of
From literature sources, find the critical temperatures for the gaseous hydrocarbons methane, ethane, propane, and butane. Explain the trends observed.
Some colloidal suspensions appear at first glance to be solutions. What quick, simple procedure could you use to distinguish colloids from solutions?
Consider an apparatus in which A and B are two 1.00-L flasks joined by a stopcock C. The volume of the stopcock is negligible. Initially, A and B are evacuated, the stopcock C is closed, and 1.50 g
A reaction mixture that consisted of 0.400 mol H2 and 1.60 mol I2 was introduced into a flask of volume 3.00 L and heated. At equilibrium, 60.0% of the hydrogen gas had reacted. What is the
Puddings contain large starch molecules that cause the mixture to thicken by a mechanism similar to that by which gelatin thickens. Which of the following suggestions is the best description of how
Calculate the equilibrium constant at 25°C for each of the following reactions, by using data in Appendix 2A: (a) the combustion (b) the oxidation 2 CO₂(g) of hydrogen: 2 H₂(g) + O₂(g) — 2
A reaction mixture that consisted of 0.20 mol N2 and 0.20 mol H2 was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of
The apparatus in Exercise 5.20 is again evacuated. Then 35.0 g of chloroform, CHCl3, is placed in flask A and 35.0 g of acetone, CH3COCH3, is placed in flask B. The system is allowed to come to
Calculate the equilibrium constant at 25°C for each of the following reactions, by using data in Appendix 2A: (a) the synthesis of trichloromethane (chloroform) from natural gas (methane). AG
The equilibrium constant Kc for the reaction 2 CO(g) + O2(g) ⇌ 2 CO2(g) is 0.66 at 2000 °C. If 0.28 g of CO and 0.032 g of O2(g) are placed in a reaction vessel of volume 2.0 L and heated to
Pentane is a liquid with a vapor pressure of 512 Torr at 25°C; at the same temperature, the vapor pressure of hexane is only 151 Torr. What composition must the liquid phase have if the gas-phase
In the Haber process for ammonia synthesis, K = 0.036 for N2(g) + 3 H2(g) ⇌ 2 NH3(g) at 500. K. If a reactor of volume 2.0 L is charged with 1.42 bar of N2 and 2.87 bar of H2, what will the
A reaction mixture consisting of 2.00 mol CO and 3.00 mol H2 is placed in a reaction vessel of volume 10.0 L and heated to 1200. K. At equilibrium, 0.478 mol CH4 was present in the system. Determine
Using a spreadsheet program or graphing calculator, plot ln P against 1/T on the same set of axes for DHvap = 15, 20., 25, and 30. kJ · mol–1 for the equation ln P = DHvap/RT. Is the vapor
A mixture consisting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed in a reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO(g)
The combustion analysis of l-carnitine, an organic compound thought to build muscle strength, reported its composition as 52.16% C, 9.38% H, 8.69% N, and 29.78% O. The osmotic pressure of 100.00 mL
A reaction mixture is prepared by mixing 0.100 mol SO2, 0.200 mol NO2, 0.100 mol NO, and 0.150 mol SO3 in a reaction vessel of volume 5.00 L. The reaction SO2(g) + NO2(g) ⇌ NO(g) + SO3(g) is
Intravenous medications are often administered in 5.0% glucose, C6H12O6(aq), by mass. What is the osmotic pressure of such solutions at 37°C (body temperature)? Assume that the density of the
In an experiment, 0.100 mol H2S is placed in a reaction vessel of volume 10.0 L and heated to 1132°C. At equilibrium, 0.0285 mol H2 is present. Calculate the value of Kc for the reaction 2 H2S(g)
When sulfuric acid is added to water, so much energy is released as heat that the solution may boil. Would you expect this solution to show a deviation from Raoult’s law? If so, which kind?Explain
Relative humidity at a particular temperature is defined asThe vapor pressure of water at various temperatures is given in Table 5A.2.(a) What is the relative humidity at 30°C when the partial
The equilibrium constant Kc = 0.56 for the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) at 250 °C. Upon analysis, 1.50 mol PCl5, 3.00 mol PCl3, and 0.500 mol Cl2 were found to be present in a reaction
At 25 °C, K = 3.2 * 10–34 for the reaction 2 HCl(g) ⇌ H2(g) + Cl2(g). If a reaction vessel of volume 1.0 L is filled with HCl at 0.22 bar, what are the equilibrium partial pressures of HCl, H2,
A dextrose/saline aqueous solution that doctors commonly use to replace fluids in the body contains 1.75 g · L–1 NaCl and 40.0 g · L–1 dextrose (C6H12O6).(a) What is the total molar
If 4.00 L of HCl(g) at 1.00 bar and 273 K and 26.0 g of I2(s) are transferred to a reaction vessel of volume 12.0 L and heated to 25°C, what will the equilibrium concentrations of HCl, HI, and Cl2
When 0.10 g of insulin is dissolved in 0.200 L of water, the osmotic pressure is 2.30 Torr at 20°C. What is the molar mass of insulin?
A reaction vessel of volume 3.00 L is filled with 0.342 mol CO(g), 0.215 mol H2(g), and 0.125 mol CH3OH(g). Equilibrium is reached in the presence of a zinc oxide–chromium(III) oxide catalyst and,
An aqueous solution of the sugar mannitol (C6H12O6) with a concentration of 180 mg · mL–1 is commonly used in veterinary medicine as an osmotic diuretic, which helps to remove water from living
For the reaction 2 NH3(g) ⇌ N2(g) + 3 H2(g), Kc = 0.395 at 350°C. A sample of NH3 of mass 25.6 g is placed in a reaction vessel of volume 5.00 L and heated to 350°C. What are the equilibrium
Human blood has an osmotic pressure relative to water of approximately 7.7 atm at body temperature (37°C). In a hospital, intravenous glucose (C6H12O6) solutions are often given. If a technician
Suppose that 0.724 mol PCl5 is placed in a reaction vessel of volume 0.500 L. What is the concentration of each substance when the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) has reached equilibrium at
Interpret the following verse from Coleridge’s Rime of the Ancient Mariner:Water, water, every where,And all the boards did shrink;Water, water every where,Nor any drop to drink.
A sample of ammonium carbamate, NH4(NH2CO2), of mass 25.0 g was placed in an evacuated flask of volume 0.250 L and kept at 25°C. At equilibrium, 17.4 mg of CO2 was present. What is the value of Kc
Dissociation of a diatomic molecule, X2 (g) ⇌ 2 X(g) occurs at 500 K. The equilibrium state of the reaction is shown in 1 and the equilibrium state in the same container after a change has
Carbon monoxide and water vapor, each at 200. Torr, were introduced into a container of volume 0.250 L. When the mixture reached equilibrium at 700°C, the partial pressure of CO2(g) was 88 Torr.
At 25°C, K = 47.9 for N2O4 (g) ⇌ 2 NO2(g).(a) If 0.180 mol N2O4 and 0.0020 mol NO2 are placed in a reaction vessel of volume 20.0 L and the reaction is allowed to reach equilibrium, what are
Consider the reaction 2 NO(g) ⇌ N2(g) + O2(g). If the initial partial pressure of NO(g) is 1.0 bar, and p is the equilibrium partial pressure of N2(g) in bar, what is the correct equilibrium
The following plot shows how the partial pressures of reactant and products vary with time for the decomposition of compound A into compounds B and C. All three compounds are gases. Use this plot to
In an experiment, 0.100 mol SO3 was introduced into a flask of volume 2.00 L and the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g) was allowed to come to equilibrium at 700 K.(a) Using information in
(a) Calculate the standard Gibbs free energies of formation of the halogen atoms X(g) at 1000. K from data available in Table 5G.2.(b) Show how these data correlate with the X—X bond strength by
Consider the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g). If the initial molar concentration of NO2(g) is 0.030 mol · L–1, and c is the equilibrium molar concentration of O2(g) in moles per liter, which

Showing 1600 - 1700 of 3011

First
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
Last

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Campus Ambassador

Company Info

Security
Copyrights
Privacy Policy
Terms & Condition
SolutionInn Fee
Scholarship

Services

Sitemap
Fun
Definitions
Become Tutor
Study Help Categories
Recent Questions
Expert Questions

Copyright © 2024 SolutionInn All Rights Reserved.

Get the SolutionInn - Study Help App