Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ  Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ  Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ    Complete the table for Reaction 3. Assume the process occurs near room temperature. Change in Enthalpy Change in Entropy Change in Gibbs Free Energy Reaction Spontaneity        ["", ""]        ["", ""]        ["", ""]        ["", ""]

The standard enthalpy change for the following reaction is -425 kJ at 298 K. K(s) + 1/2O₂(g) + 1/2 H₂(g) →→→ KOH(s) ΔΗ AH° = -425 kJ What is the standard enthalpy change for the reaction at 298 K? 2 K(s) + O₂(g) + H₂(g) – 2 KOH(s) kj Submit Answer Retry Entire Group 9 more group attempts remaining

Determine the heat involved in the combustion of liquid hydrazine by using the following reactions. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ)      ΔH°= –1013 kJ/molN2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ)      ΔH°= –317 kJ/mol2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ)      ΔH°= –142.9 kJ/molH2(g) + ½ O2(g) → H2O(ℓ)       ΔH°= –285.8 kJ/mol Then, Launching a small spacecraft to study Jupiter required approximately 28 million kJ. Assume that hydrazine was the only fuel. What mass of hydrazine, in kilograms, was needed for the launch?

What is the enthalpy change when  2.00 mol of oxygen (O2) react? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ

Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCI(g) AH = –184.6 kJ Reaction 2: 20F2(g) O2(8) + 2 F2(g) AH: -49.4 kJ Reaction 3: N2(8) + 202(8) - 2NO2(g) ΔΗ+66.4 kJ

Consider the reaction: 4A + B= 2C.        Δ H=-443.6Kj/mol what reaction corresponds to a H of Δ221.8 Kj/mol

The reaction below is a  exothermic or endothermic reaction. 2SO3(g) + Heat ⇋ 2SO2(g) + O2(g)

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)   3 C(s) + 4 H2(g) → C3H8(g)           ΔH = – 118.2 kJ C(s) + O2(g) → CO2(g)                   ΔH = – 62.4 kJ H2(g) + 1/2 O2(g) →  H2O(g)          ΔH = – 182.5 kJ

（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?

Consider the reaction: 8 H2O (l) + 4CO2 (g)→4  CH3OH (l) + 6 O2 (g) ΔH = +2905.6 kJ What is ΔH for the following reaction? 2 CH3OH (l) + 3 O2 (g) →4 H2O (l) + 2 CO2 (g)