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A chemistry student wants to understand the effect of changing the volume on the equilibrium position of a chemical reaction. Accordingly, the student designs an experiment where they mix 0.2 mol of nitrogen gas with 0.1 mol of hydrogen gas in a 1 L container and allow them to react to form ammonia gas. If the reaction reaches equilibrium at a certain temperature and the volume of the container is suddenly decreased to 0.5 L, what will be the effect on the concentration of ammonia gas?

asked Jan 22 in Chemical equilibrium by Makayla14235 (2.3k points)

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Calculate the final temperature when 25 grams of aluminum at 80°C is placed in 100 grams of water at 25°C. The specific heat capacity of aluminum is 0.90 J/g°C and the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by Sterling80B (2.1k points)

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Calculate the enthalpy change for the polymerization of 2-methyl-1,3-butadiene (MBC) if 1 mole of MBC is polymerized in a perfectly insulated container at a constant temperature of 25°C. The reaction equation for the polymerization of MBC is given as:nC5H8 (MBC) → (C5H8) (Polymer)Given the bond dissociation energies (in kJ/mol) for the following bonds:C-C bond = 348C-H bond = 413Assume that the enthalpy change of vaporization of MBC is negligible.

asked Jan 23 in ThermoChemistry by SusannahCrow (2.4k points)

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Calculate the extent of polarization for a cell in which a copper electrode is coupled with a silver electrode at 25°C. The copper electrode has a potential of -0.34 V and the silver electrode has a potential of 0.80 V. The initial concentration of copper ions and silver ions in the solution are 0.001 M and 0.01 M, respectively. The total resistance of the cell (including both the electrolyte and the external circuit) is 10 ohms. Assume that the transfer coefficient for both the copper and silver ions is 0.5, and the Faraday constant is 96,485 C/mol.

asked Jan 23 in ElectroChemistry by RogerDenning (2.4k points)

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1 answer 56 views

Calculate the entropy change (∆S) for the reaction of 2 moles of solid NH4Cl with 1 mole of NaOH in a coffee cup calorimeter at a constant temperature of 25°C. The reaction takes place in 100 mL of water and produces 2 moles of NH3 and 1 mole of NaCl in solution. Assume that the specific heat capacity of water is 4.18 J/g·K and that the final solution temperature after the reaction is complete is 25°C.

asked Jan 23 in Chemical thermodynamics by GlendaNester (1.8k points)

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1 answer 70 views

Calculate the bond dissociation energy (in kJ/mol) of chlorine gas (Cl2) if it requires 243 kJ of energy to break a single Cl-Cl bond in the gas phase.

asked Jan 23 in ThermoChemistry by AlineBacon1 (1.5k points)

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1 answer 69 views

Calculate the bond order and bond length of the nitrogen-oxygen bond in the molecule NO.

asked Jan 23 in Inorganic Chemistry by EvieOconnor (2.3k points)

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Calculate the enthalpy of combustion of methane if 2.56 g of methane was burnt completely in a bomb calorimeter containing excess oxygen, causing a temperature rise of 4.58 °C in the calorimeter, which has a heat capacity of 1.26 kJ/°C. The balanced chemical equation for the combustion of methane is as follows: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) + energy.

asked Jan 23 in ThermoChemistry by MaxwellDuff3 (1.9k points)

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Calculate the enthalpy change of dissolving 5.00 g of NaOH in 100.0 g of water. The temperature of the resulting solution increases from 25.00°C to 31.50°C. The specific heat capacity of the resulting solution is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by EloisaPtm353 (1.9k points)

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1 answer 55 views

Calculate the equilibrium constant for the reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) if at equilibrium the concentrations are [NOCl] = 0.050 M, [NO] = 0.030 M, and [Cl2] = 0.020 M.

asked Jan 23 in Chemical equilibrium by SNBBernd7967 (2.3k points)

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1 answer 103 views

A laboratory made a buffer solution by mixing 25 mL of 0.10 M acetic acid (Ka = 1.8 x 10^-5) with 15 mL of 0.20 M sodium acetate solution. Calculate the pH of the buffer solution assuming both the acid and the acetate ions are completely dissociated.

asked Jan 22 in Chemical reactions by OrenDarwin6 (1.9k points)

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1 answer 109 views

A chemistry student is provided with 10 grams of copper oxide and 5 grams of magnesium. The student reacts the two substances to form copper and magnesium oxide. What is the limiting reactant in this reaction and how many grams of copper can be produced?

asked Jan 22 in Chemical reactions by EloisaPtm353 (1.9k points)

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1 answer 60 views

Calculate the enthalpy of ionization of magnesium if 4.8 g of magnesium reacts completely with hydrochloric acid to form 224 mL of hydrogen gas at standard temperature and pressure (STP). The heat released during the reaction is -412 kJ/mol.

asked Jan 23 in ThermoChemistry by AudreaV25265 (2.0k points)

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1 answer 62 views

Calculate the enthalpy of adsorption of 1 mole of hydrogen gas on the surface of activated charcoal from the given data:- The heat of combustion of hydrogen gas at constant volume is -285.8 kJ/mol- The heat of combustion of hydrogen gas at constant pressure is -241.8 kJ/mol- The heat of vaporization of hydrogen gas at its boiling point (20.3 K) is 0.452 kJ/mol- The surface area of activated charcoal is 500 m²/g- The weight of activated charcoal used is 0.5 g.

asked Jan 23 in ThermoChemistry by BradConger9 (1.8k points)

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1 answer 67 views

Calculate the electrical double layer thickness of a silica particle with a radius of 50 nm, assuming the particle is in water at room temperature and has a surface charge density of -0.05 C/m².

asked Jan 23 in Physical Chemistry by AstridMusser (1.9k points)

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1 answer 63 views

Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l) using Hess's law given the following reactions: 2H2(g) + O2(g) → 2H2O(g) ΔH1 = -483.6 kJ/mol 2H2O(g) → 2H2O(l) ΔH2 = -40.7 kJ/mol

asked Jan 23 in ThermoChemistry by KrystleDHage (2.0k points)

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1 answer 55 views

Calculate the equilibrium constant (K) of the electrochemical reaction below at 25°C: 2AgCl(s) + H2(g) <--> 2Ag(s) + 2HCl(aq) Given: E°AgCl/Ag = 0.22 V E°HCl/H2 = 0.00 V Kw = 1.0 x 10^-14 at 25°C Standard Hydrogen Electrode (SHE) has E° = 0.00 V

asked Jan 23 in ElectroChemistry by QJXClarice2 (2.5k points)

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1 answer 64 views

Calculate the enthalpy change for the following polymerization reaction: 2 C2H4 (g) → C4H8 (g) Given the following bond enthalpies: C-H = 413 kJ/mol, C-C = 348 kJ/mol, C=C = 611 kJ/mol Assume all reactants and products are gases at 298 K and 1 atm.

asked Jan 23 in ThermoChemistry by AntonyKnotts (1.8k points)

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Calculate the equilibrium constant (K) for the reaction between copper and silver ions in a galvanic cell at room temperature (25°C), given the following half-reactions and their respective reduction potentials:Cu2+ (aq) + 2e- → Cu (s) E°red = +0.34 VAg+ (aq) + e- → Ag (s) E°red = +0.80 VAlso, if the cell is constructed with a copper electrode and a silver electrode, which electrode will be the cathode and which will be the anode?

asked Jan 23 in ElectroChemistry by RandellBeggs (2.0k points)

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1 answer 63 views

Calculate the enthalpy change for the reaction below using the given bond dissociation energies:2HBr (g) + Cl2 (g) -> 2HCl (g) + Br2 (g)Bond dissociation energies:H-H = 436 kJ/molBr-Br = 193 kJ/molH-Br = 366 kJ/molCl-Cl = 242 kJ/molH-Cl = 431 kJ/mol

asked Jan 23 in Chemical reactions by AugustBranno (2.5k points)

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