Ammonia reacts with oxygen as follows: 4NH3(g) + 702(g) → 4NO2(g) + 6H20(g) AH° = -1132 kJ Calculate the enthalpy change for the combustion of 7.76 mol of NH3. kJ
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- 9.63 Reactions of hydrocarhons are often studied in the petroleum industry. One example is 2C3H8(g)C6H6(l)+5H2(g) , with H = 698 kJ. If 35 L of propane at 25C and 0.97 atm is to be reacted, how much heat must he supplied?Liquid trinitroglycerin (C3H5N3O9) has been widely used as an explosive and as a medication to relieve angina. The enthalpy of decomposition (ΔHdec) for C3H5N3O9 to form N2(g), CO2(g), H2O(l), and O2(g) is -1541.4 kJ/mol. 1. Write the thermochemical equation for the decomposition of 1 mole of trinitroglycerin. 2. Calculate the standard heat of formation (ΔHf) for C3H5N3O9. 3. A standard does of C3H5N3O9 for relief of angina is 0.60 mg. If a sample is eventually oxidized completely, how many calories are released?When H2S(g) reacts with H2O(l) to form H2(g) and SO2(g), 295 kJ of energy are absorbed for each mole of H2S(g) that reacts.Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive.Use the SMALLEST INTEGER coefficients possible and put the energy term in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. + + + +
- Given the following enthalpies of combustion: (a) 2H2(g) + O2(g) --> 2H2O(g); DH = -483.6 kJ (b) 2C3H6(g) + 9O2(g) --> 6CO2(g) + 6H2O(g); DH = -3853.6 kJ (c) C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(l); DH = -2043.7 kJ Calculate DH for the following reaction: (A 4) C3H6(g) + H2(g) --> C3H8(g) (A) -124.9 kJ (B) -366.7 kJ (C) -2293.5 kJ (D) -4262.3kJPlease help me with my hw. Tysm❤️ ACTIVITY: Answer completely. Calculate the standard enthalpies of combustion at 25ᵒC of the following: (a) C4H8(g) + H2(g) à C4H10(g)ΔHᵒ = -2878.6kJ (b)C4H6(g) + 2H2(g) à C4H10(g)ΔHᵒ = -2543.5 kJGiven that the heat of formation for AgNO3 (s) is -124.4 kJ/mol, At standard conditions, what is dH when 56g of AgNO3 (M = 169.9 g/mol) reacts?
- Calculate the heat of reaction, Hrxn, for the combustion of one mole of C6H6(l) using the ∆reactions provided below. 6 C(s, graphite) + 3 H2(g) → C6H6(l) ∆H = 49.0 kJ H2(g) + ½ O2(g) → H2O(l) ∆H = -285.8 kJ∆ C(s, graphite) + O2(g) → CO2(g) ∆H = -393.5 kJ I've attached a photo for more clarity. Thanks!When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 751 mm Hg? Please put answer in kJ not kJ/mol. ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05The ΔHreaction for the combustion of ethanol (CH3CH2OH) is -1,370.7 kJ/mol. If 100.0 g of ethanol (CH3CH2OH) reacts with 3.000 X 1024 molecules of oxygen gas, how kJ of heat will be released? Show work/to really explain approach please.
- What quantity of heat (in kJ) will be released (∆H) if 0.4501 mol of NH3, are mixed with O.200 mol of O2 in the following chemical reaction? 4 NH3 (g) +O2 (g)→ 2 N2H4(g) +2 H2O (g) ∆ H° = -286 kJ/molWrite a balanced equation for the combustion of CH3C6H13(l) (methyl hexane)-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of CH3C6H13(l) is -173.0 kJ/mol What is the standard heat of reaction (ΔH°) for the combustion reaction of CH3C6H13(l)? Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methyl hexane. (Assume standard state conditions and 298 K for all reactants and products.)The enthalpy for combustion for ethanol at 298 K is -1370.7 kJ/mole and occurs via the following balance chemical reaction. C2H6O (l) + 3 O2 (g) ⟶ 2 CO2 (g) + 3 H2O (g) If 0.461 grams of ethanol are combusted in the presence of 1.28 g of O2, answer the following. a. How many grams of CO2 could be produced? b. How much heat is released? c. What is the change in internal energy (ΔU)?