(2) Given: compound DH°, (KJ/mol) H,O,(1) - 187.7 H,O(1) - 285.5 (a) Calculate the standard heat of reaction, H°, 2 H,O,(1) ----> 2 H,O(1)+ 0,(g), for rexn, (b) Use IG° = [H° -TÖDS° to predict whether the above reaction will be spontaneous or nonspontaneous at standard state.

How do I find the kJ?

11. answer question in pic pls

Syngas can be burned directly or converted to methanol. Calculate AH° for the reaction CO(g) + 2H, (g) → CH3OH(1) You may need to use the following data: Eompound H; (kJ/mol) H2 (g) CH3OH(1) -239 CO(g) -110.5 AH kJ

2) Consider the situation: 2CH,O, + 30) 4H,0 + e) AH --1453.0 kJ 2 CO, ΔΗ, 2(8) Showing your work, how much heat would this represent for the combustion of 12.74 mol of liquid methanol (CH4O0)? Answer to 1 decimal place. [K3] the follouing processes: (2 marks each) [C4]

3 C2H2(g) → CHo(g) What is the standard enthalphy change AH°, for the reaction represented above? (AH®7of C2H2(g) is 230 kJ mol-1; (AH®5of €CGH6(g) is 83 kJ mol-1:) (A) -607 kJ (B) -147 kJ (C) (C) -19 kJ (D) +19 kJ (E) +773 kJ

The reaction between hydrogen and oxygen to yield water vapor has AH" = -1843 2H₂(g) + O₂(g) 2H₂O(g)AH <=-484kJ Part A What is the enthalpy change in kilojoules when 0.70 mol of H₂ reacts with 0.35 mol of O, to produce 0.70 mol of H₂ at constant pressure of 1.00 atm? Express your answer as a whole number. AH = Submit Part B W= Submit 1957 ΑΣΦ How much PV work is done in kilojoules for this reaction at constant pressure of 1.00 atm if the volume change is-9-2 L? Express your answer using two significant figures. 100 ΑΣΦΑ Part C Request Answer Request Answer kJ What is the value of AE for this reaction in kilojoules?

3. The enthalpy change of a reaction Hrxn equals heat q, if the reaction is performed ... (A) in a closed system (B) in an isolated system (C) at constant volume (D) at constant temperature (E) at constant pressure