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Calculate the enthalpy change for the combustion of methane gas if 10 grams of methane is burned completely in the presence of excess oxygen gas. Given the following balanced chemical equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)The standard enthalpy of formation for methane gas is -74.8 kJ/mol, carbon dioxide gas is -393.5 kJ/mol, and water vapor is -241.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by Hulda4183859 (2.2k points)

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Calculate the cell potential for the following electrochemical reaction at 25°C: Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) Given: E°(Ag+/Ag) = +0.80 V E°(Zn2+/Zn) = −0.76 V

asked Jan 23 in ElectroChemistry by Lynell160113 (1.8k points)

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Calculate the formal charge of nitrogen in the nitrogen dioxide (NO2) molecule.

asked Jan 23 in Inorganic Chemistry by AubreyWoore (2.4k points)

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Calculate the bond order and bond length of the nitrogen-oxygen bond present in the nitrate ion (NO3-).

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

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1 answer 114 views

A chemistry experiment involves burning a sample of propane gas, C3H8, and measuring the heat released. If 2.00 grams of propane is burned completely to produce CO2(g) and H2O(l), and the heat of combustion is found to be -2044 kJ/mol, what is the heat released in kJ when 2.00 grams of propane is burned?

asked Jan 22 in ThermoChemistry by SteveAdamson (1.7k points)

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Calculate the enthalpy change (ΔH) for the isomerization of butene-1 to butene-2, given that the heat of combustion of butene-1 and butene-2 are -2657.7 kJ/mol and -2674.4 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by LeifLeverett (2.3k points)

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1 answer 67 views

Calculate the enthalpy change of isomerization for the conversion of cis-but-2-ene to trans-but-2-ene, given the standard enthalpy of formation for both isomers. Asssume all other conditions remain constant.

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

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1 answer 105 views

A student is given a galvanic cell consisting of a zinc electrode and a copper electrode. If the concentration of zinc ions in the zinc half-cell is 0.1 M and the concentration of copper ions in the copper half-cell is 1.0 M, what is the corrosion potential of the zinc electrode at standard conditions? (Assume that the standard electrode potential of copper is +0.34 V and that of zinc is -0.76 V.)

asked Jan 22 in ElectroChemistry by AdeleStrothe (2.1k points)

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Calculate the activation energy for the following electrochemical reaction: 2H₂O(l) → O₂(g) + 4H⁺(aq) + 4e⁻ if the half-cell potentials are: E°(O₂/H₂O) = 1.23 V E°(H⁺/H₂) = 0 V Assuming the reaction follows Arrhenius equation, where the rate constant k is related to the activation energy Ea, temperature T and pre-exponential factor A by: k = A exp(-Ea/RT) where R is the gas constant equal to 8.314 J/molK.

asked Jan 23 in ElectroChemistry by ShaunBehan45 (2.8k points)

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Calculate the change in entropy when 1 mole of methane gas (CH4) is burned completely in oxygen gas (O2) at constant pressure and 298 K.

asked Jan 23 in Chemical thermodynamics by CharleneLemu (1.7k points)

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1 answer 73 views

Calculate the bond length between a fluorine atom (F) and a carbon atom (C) in a molecule of CF4, given that the bond energy is 544 kJ/mol and the force constant is 455 N/m.

asked Jan 23 in Chemical bonding by EdgardoHinch (2.2k points)

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1 answer 64 views

Calculate the enthalpy of formation of So₃(g) using the given thermochemical equations:2SO₂(g) + O₂(g) → 2SO₃(g) ∆H = -197 kJ/mol2SO₂(g) + 2O₂(g) → 2SO₃(g) ∆H = -792 kJ/mol

asked Jan 23 in ThermoChemistry by BradCoz53277 (1.9k points)

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1 answer 113 views

A chemistry student is given a sample of a compound containing sulfur, oxygen, and carbon. The student needs to determine the mass percentages of each element in the compound using mass balance calculations. The sample has a total mass of 5.00 grams, and the student devises an experiment to isolate each of the three elements by chemical reactions, and the mass of each element is recorded as follows: 1.20 g sulfur, 1.80 g oxygen, and 2.00 g carbon. What are the mass percentages of sulfur, oxygen, and carbon in the compound?

asked Jan 22 in Analytical Chemistry by RosettaMcinn (1.7k points)

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1 answer 71 views

Calculate the corrosion rate of an iron rod with a surface area of 20 cm² that is connected to a copper plate with a surface area of 25 cm², immersed in a solution of 0.5 M copper sulfate, given that the measured current is 0.2 A.

asked Jan 23 in ElectroChemistry by DebFannin623 (1.8k points)

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1 answer 104 views

A student mixed 0.1 M solution of NH3 and 0.1 M solution of NH4Cl to form a buffer solution of NH3/NH4+. If the initial pH of the solution is 9.25, what will be the final pH of the solution when 0.01 moles of HCl is added? (Assume the volume of the solution is constant).

asked Jan 22 in Chemical equilibrium by HoraceT7712 (2.0k points)

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1 answer 100 views

A student wants to investigate the effect of volume change on the equilibrium position of the reaction 2SO2(g) + O2(g) ⇄ 2SO3(g). The initial equilibrium concentration of SO3 is 0.1 M at a constant temperature. The volume is reduced by half at equilibrium. Calculate the new equilibrium concentrations of SO2, O2 and SO3 assuming the equilibrium constant (Kc) of the reaction remains constant.

asked Jan 22 in Chemical equilibrium by KreogMoore5 (6.4k points)

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Calculate the bond dissociation energy (in kJ/mol) of the C-H bond in methane (CH4) using the following data: - The enthalpy change for the combustion of one mole of methane gas is -890.3 kJ/mol.- The energy required to break one mole of H-H bonds is 433.4 kJ/mol.- The energy required to break one mole of C=O bonds is 799.5 kJ/mol.- The energy required to break one mole of O-H bonds is 463.0 kJ/mol.

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

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1 answer 57 views

Calculate the heat of crystallization (in kJ/mol) of NaOH if 25g of NaOH dissolves in 100g of water at 25°C and releases 4.75kJ of heat.

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

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1 answer 63 views

Calculate the enthalpy of reduction for Fe2O3 given that it is reduced to FeO by hydrogen at 298K and constant pressure. Given that the standard enthalpy of formation of Fe2O3 and FeO are -822kJ/mol and -272kJ/mol respectively, the heat of combustion of hydrogen is -286kJ/mol and the enthalpy of formation of H2O is -285.8kJ/mol.

asked Jan 23 in ThermoChemistry by LethaWinfrey (1.7k points)

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1 answer 70 views

Calculate the enthalpy change (in kJ/mol) for the isomerization reaction of butene-1 to butene-2. Given the standard enthalpy of formation values for butene-1 as -126.3 kJ/mol and butene-2 as -126.0 kJ/mol, and the heat of combustion values for butene-1 as -2670.0 kJ/mol and butene-2 as -2666.0 kJ/mol.

asked Jan 23 in ThermoChemistry by DanieleLane (1.6k points)

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