Identify the reaction below for which ΔH°rxn = ΔH°f; i.e., which equation below gives ΔH°f, the standard enthalpy of formation for glucose, C6H12O6(s): Group of answer choices 6 C(s)  +  12 H(g)  +  6 O(g)   →   C6H12O6(s) 6 C(g)  +  6 H2(g)  +  3 O2(g)   →   C6H12O6(s) 2 C2H5OH(l)  +  2 CO2

Sketch an enthalpy diagram for the combustion of cyclopropane, C3H6 (g).

The reaction written below has a ΔH of +2,971 kJ          6CO2(g) + 6H2O(g) --> C6H12O6(g) +6O2(g) How much energy must be input into this reaction to make 93.087 grams of C6H12O6(g) ?  (Input your answer in kJ, but do not include the units in your answer.)

Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + 2H2(g) C2H4(g) AH° = 52.3 kJ (2) 2C(s) + 3H2(g) C2H6(g) AH° = -84.7 kJ what is the standard enthalpy change for the reaction: (3) C2H4(g) + H2(g) C2H6(g) AH° = ? kJ

The oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/mol

Calculate ΔHrxn for the reaction: 7 C (s) + 8 H2 (g) → C7H16 (g) The following reactions and associated ΔHrxn values are may likely be helpful to you: Reaction A: C7H16(g) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (g) ΔHrxn = -4817 kJ Reaction B: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ Reaction C: 2 H2 (g) + O2 (g) → 2 H2O (g) ΔHrxn = -483.6 kJ

The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04

A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 302(g) →2 KClO3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction ΔΗ ㅁ x10 2K C103 (s) → 2KC1(s) + 302(g) KCIO, (s)-KCI(s) + 0,(s) 3 KCI(s)+0, (g)KCIO, (s) kJ kJ 1 5

The balanced thermochemical equation for the combustion of exactly one mole of propane is: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O(l) ΔH = -2220 kJ/mol What is the enthalpy change for the reaction: 1.5 CO2 (g) + 2 H2O(l)  → 0.5 C3H8 (g) + 2.5 O2 (g) ΔH = ?

（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g)     ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A?   （2）Consider the reaction: C (s) + O2 (g) → CO2 (g)     ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?