The Martian In the motion picture The Martian, a stranded astronaut uses hydrazine, N,H4, to produce hydrogen, which he then reacts with oxygen to make water. The enthalpy of the reaction between N,H, and O2 is AHn -622 kJ/mol. Calculate the standard enthalpy of formation of N,H,(e) from the standard enthalpy changes of the following reactions: N,H,(e) + O2(g)→ N2(g) + 2 H,0(g) AHn = -622 kJ %3D rxn H;(g) +} 0,(g) → H,O(g) AHxn = -285.8 kJ %3D N2(g) + 2 H2(g) - N,H,(€) AHn = ? L %3D rxn

Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84

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

In the laboratory, a student dilutes 17.8 mL of a 9.80 M hydrobromic acid solution to a total volume of 125.0 mL. What is the concentration of the diluted solution? Concentration = 0.78 M

Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -103.2 kJ: 4HCl(g) + O2(g) → 2H₂O(g) + 2Cl₂ (g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(g) is I kJ/mol red Species AH (kJ/mol) H₂O(g) -241.8 Cl₂(g) 0.0 0₂ (9) 0.0

Calculate the enthalpy of formation of 1 mole SO₂(g) from the standard enthalpy changes of the following reactions: 2SO3(g)2SO₂(g) + O₂(g) 2S (s) +30₂(g) → 2SO3(g) →→ SO₂(g) S(s) + O₂(g) kJ ΔΗ AH rxn 1=+196 kJ rxn 2 = -790 kJ AHO rxn 3 = ? k

A scientist measures the standard enthalpy change for the following reaction to be -912.5 kJ:2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is  kJ/mol.

（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?