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Consider the following reaction: 2 SO2(g) + O2(g) ⇌ 2SO3(g) ΔH = -198 kJ/mol What will be the effect on the equilibrium concentration of SO3 if:a) The pressure of the system is increased?b) The concentration of SO2 is increased?c) A catalyst is added to the system?

asked 6 days ago in Chemical reactions by DorcasBlaylo (690 points)

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Calculate the mass of sodium chloride (NaCl) produced when 2.5 moles of sodium (Na) react completely with excess chlorine gas (Cl2). (Hint: Use the balanced chemical equation 2Na + Cl2 → 2NaCl)

asked Jan 23 in Chemical reactions by SOZIsmael446 (350 points)

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Calculate the equilibrium constant (Kc) of the chemical reaction: 2NOCl(g) ⇌ 2NO(g) + Cl2(g) where the concentration of NOCl is 0.5 M, NO is 0.2 M, and Cl2 is 0.1 M at equilibrium at a certain temperature.

asked Jan 23 in Chemical reactions by MarielKeble (1.1k points)

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Calculate the equilibrium constant (Kc) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) if the equilibrium concentration of nitrogen (N2) is 0.025 M, hydrogen (H2) is 0.10 M, and ammonia (NH3) is 0.015 M.

asked Jan 23 in Chemical reactions by Wendell4581 (470 points)

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Calculate the enthalpy change when 50 mL of 2 M HCl solution reacts with excess NaOH according to the balanced chemical equation: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) Given that the specific heat capacity of the solution is 4.18 J/g°C, and the initial and final temperatures of the solution are 25°C and 35°C, respectively. Assume a density of 1 g/mL for the solution.

asked Jan 23 in Chemical reactions by JustineDez22 (470 points)

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Calculate the enthalpy change of the following chemical reaction: 2H2 + O2 → 2H2O Given: - ΔHf°(H2O) = -286 kJ/mol - ΔHf°(H2) = 0 kJ/mol - ΔHf°(O2) = 0 kJ/mol

asked Jan 23 in Chemical reactions by CallieMargar (550 points)

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Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) --> 2H2O(g) given the following enthalpy changes: H2(g) + 1/2O2(g) --> H2O(g) ΔH1 = -286 kJ/molH2(g) + 1/2Cl2(g) --> HCl(g) ΔH2 = -92 kJ/mol Cl2(g) --> 2Cl(g) ΔH3 = +242 kJ/molHCl(g) + 1/2O2(g) --> H2O(g) + Cl2(g) ΔH4 = -184 kJ/mol

asked Jan 23 in Chemical reactions by LinoShearer (530 points)

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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 JoieO4733186 (690 points)

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Calculate the enthalpy change for the following reaction:2H2O2(aq) → 2H2O(l) + O2(g)Using the following information:2H2O(l) + 105.2 kJ → 2H2(g) + O2(g)2H2(g) + O2(g) → 2H2O2(aq) + 484.4 kJ

asked Jan 23 in Chemical reactions by KristoferHol (830 points)

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Calculate the enthalpy change for the following reaction, using Hess's Law:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following enthalpy changes: 2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ2SO2(g) + O2(g) → 2SO3(g) ΔH2 = -198 kJ2H2(g) + S(s) → H2S(g) ΔH3 = +25kJ

asked Jan 23 in Chemical reactions by ColinBatty1 (450 points)

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Calculate the enthalpy change for the following reaction using Hess's Law: 2SO3(g) → 2SO2(g) + O2(g)Given the following enthalpy changes:2SO3(g) + ΔH1 → 2SO2(g) + O2(g); ΔH1 = 198.2 kJ/molSO2(g) + 1/2O2(g) + ΔH2 → SO3(g); ΔH2 = -98.9 kJ/mol

asked Jan 23 in Chemical reactions by RodDeboer029 (430 points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) if 37.0 g of CH4 is completely burned in a bomb calorimeter and the temperature increases by 285.4 K. Assume that the calorimeter has a heat capacity of 4.40 kJ/K and that the combustion reaction is as follows: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l); ΔH=-890.4 kJ/mol. What is the enthalpy change for the combustion of one mole of methane gas?

asked Jan 23 in Chemical reactions by AudryCastle (550 points)

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Calculate the enthalpy change for the combustion of methane at standard conditions, given the following information:- The enthalpy of formation of CO2(g) is -393.5 kJ/mol.- The enthalpy of formation of H2O(g) is -241.8 kJ/mol.- The enthalpy of formation of CH4(g) is -74.8 kJ/mol.

asked Jan 23 in Chemical reactions by ThereseRosso (750 points)

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Calculate the enthalpy change for the combustion of methane (CH4) at constant pressure, given that the heat of formation for methane is -74.9 kJ/mol and the balanced chemical equation is: CH4 (g) + 2O2 (g) -> CO2 (g) + 2H2O (l) The heat of formation for CO2 is -393.5 kJ/mol and the heat of formation for H2O is -285.8 kJ/mol.

asked Jan 23 in Chemical reactions by DoyleLehman (360 points)

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Calculate the enthalpy change for the combustion of 5.67 grams of methane (CH4) if the standard enthalpy of combustion of methane is -890.4 kJ/mol.

asked Jan 23 in Chemical reactions by FCRJohnnie31 (590 points)

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Calculate the energy required to break all the bonds in 1 mole of methane gas (CH4) at standard conditions, given that the bond energies of C-H and C-C bonds are 413 kJ/mol and 348 kJ/mol, respectively. Then, calculate the total energy released or absorbed during the combustion of 1 mole of methane gas with oxygen gas to form carbon dioxide gas and water vapor.

asked Jan 23 in Chemical reactions by Antoinette08 (510 points)

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Calculate the energy required to break a carbon-carbon single bond (C-C) with a bond length of 1.54 Å using the average bond-dissociation energy of 347 kJ/mol for this type of bond.

asked Jan 23 in Chemical reactions by StewartLivin (490 points)

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Calculate the direction in which the equilibrium position will shift for the following reaction if the pressure is increased: N2(g) + 3H2(g) ⇌ 2NH3(g) ∆H° = -92.4 kJ/mol. Use Le Chatelier's principle to justify your answer.

asked Jan 23 in Chemical reactions by JannaNormanb (650 points)

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Calculate the change in enthalpy for the following chemical reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given that the enthalpies of formation for CH4(g), CO2(g), and H2O(l) are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol respectively.

asked Jan 23 in Chemical reactions by CharlesMagil (290 points)

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1 answer 48 views

Calculate the change in enthalpy (ΔH) for the combustion of 10 grams of propane (C3H8) if the heat released by the reaction is -2202 kJ.

asked Jan 23 in Chemical reactions by LuellaHenn7 (450 points)

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