Table sugar (sucrose) is hydrolyzed to form glucose (a simple sugar) according to the following equation: C12H22011 (s) +H,0(g) → 2C,H1,0g(s) Determine the enthalpy change for the hydrolysis reaction given the following information: C12H22011(s) + 120,(g) 12CO, (g) + 11H,0(g) > ΔΗ = -5640 kJ rxn CH1206(s) + 602(g) → 6C0,(g) + 6H0(g) > 12°6 ΔΗ. = -2800 kJ rxn kJ

Consider these reactions, where M represents a generic metal. 2 M(s) + 6HCl(aq) →→→ 2 MC1₂(aq) + 3H₂(g) HCI(g) HCl(aq) H₂(g) + Cl₂(g) → 2 HCI(g) MCI, (s) → MCI, (aq) Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl₂(g) → 2 MC1₂ (s) 1. 2. 3. 4. ΔΗ = AH₁ = -694.0 kJ AH₂ = -74.8 kJ AH3= -1845.0 kJ AH4 = -375.0 kJ kJ

Combustion of a hydrocarbon, X, is given by the equation: 2 X + 5 O2 (g) --> 4 CO2 (g) + 6 H2O (g)           ∆H = -75.0 kJ Determine the standard enthalpy of formation of the hydrocarbon, X.

When 6.10 g of urea,(NH2)2CO (g), burns to produce CO2 (g), N2 (g) and H2O (l) 67.8 kJ of heat energy are released in a bomb calorimeter.  What is the energy released in the burning of one mole of urea?  Using this, what is the enthalpy of formation of urea?

Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = 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

Consider these reactions, where M represents a generic metal. 2 M(s) + 6HCl(aq) 2 MC13(aq) + 3H₂(g) HCl(g) HCl(aq) H₂(g) + Cl₂ (g) - MC13 (s) →→→ MC1₂ (aq) Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl₂(g) → 2 MC1₂ (s) 1. 2. 3. 4. AH = 2 HCl(g) AH₁ = -553.0 kJ ΔΗ, = −74.8 kJ AH3 = -1845.0 kJ AH4 = -337.0 kJ kJ

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

1 If the standard enthalpy of cembustion of gaseous cyclopropane, C3H6, is -2091.2 kJ mol- at 25 C, calculate the standard enthalpy of formation of the compound at 298 K. (The standard enthalpy of combustion is the heat of combustion of one mole of a compound to the most stable combustion products, which are CO2(g) and H20(1) in the case of hydrocarbons. The standard enthalpy of formation is the enthalpy of formation of one mole of a compound from its constituent elements, the compound and its constituent elements in their standard states.)

A scientist measures the standard enthalpy change for the following reaction to be 79.4 kJ:NH4Cl(aq)NH3(g) + HCl(aq)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(aq) is  kJ/mol.