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- Enter your answer in the provided box. You are given the following data: H,(g) → 2H(g) AH° = 436.4 kJ/mol Br2(g) → 2Br(g) AH° = 192.5 kJ/mol H;(g) + Br2(g) → 2HB1(g) AH° = -72.4 kJ/mol Calculate AH for the reaction H(g) + Br(g) → HBr(g) kJ/molarrow_forwardCalculate the heat of reaction, ▲H°, for this conversion.arrow_forwardCalculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N20(g) → 4N2(g) + 3H2O(1) AH = –1010. kJ N20(g) + 3H2 (9) → N¿H4(1)+H2O(1) AH = -317 kJ N2H4 (1) + O2 (g) → N2(g)+ 2H2O(1) AH = -623 kJ H2 (9) + 02 (9) → H2O(1) AH = -286 kJ ΔΗ - kJarrow_forward
- CH3OH (l) + 3/2 O2 (g) → CO2 (g) + 2 H2O (l), ΔH = -726.4 KJ/mol C (graphite) + O2 (g) → CO2 (g), ΔH = - 393.5 KJ/mol H2 (g) + ½ O2 (g) → H2O (l), ΔH = - 285.8 KJ/mol Calculate the enthalpy of formation of methanol from its elements: C (graphite) + 2 H2 (g) + ½ O2 (g) → CH3OH (l)arrow_forwardCalculate ΔH° for each reaction. a. HO• + CH4 → •CH3 + H2O b. CH3OH + HBr → CH3Br + H2Oarrow_forwardUse the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g) + I2(g) → CH3I(g) + HI(g) ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H 413 , C - I 240 , H - I 299 , I - I 151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.arrow_forward
- Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + H₂(g) → C₂H₂ (9) AH° = 226.7 kJ (2) 2C(s) + 2H₂(g) → C₂H₁ (9) ΔΗ° = 52.3 kJ What is the standard enthalpy change for the following reaction? (3) C₂H₂(g) + H2 (9) → C2H4 (9) AH° =? Standard enthalpy change = kJarrow_forwardCalculate the heat energy (ΔHreaction) produced when 1 mole of ethanol burns to produce CO2 and H2O as given below: C2H5OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (l)arrow_forwardThe enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/molarrow_forward
- Use the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJIf 49.9 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 30100 J of energy assuming that there is excess nitrogen and oxygen? Determine the heat of reaction in kJ for the reaction below.3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) ΔH =arrow_forwardUse the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJ If 35.5 g of NO g is reacted with excess oxygen, how much heat energy is produced?arrow_forwardUse the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJIf 57.4 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 39600 J of energy assuming that there is excess nitrogen and oxygen? Determine the heat of reaction in kJ for the reaction below.3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning