Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H₂(g)+ O₂(g)→ H₂O(l); ΔH = -285.8 kJ A)Per mole of O₂,the change in enthalpy is -571.6 kJ. B)The value -571.6 kJ pertains to 1 mol of liquid water. C)If the equation is reversed,ΔH becomes +285.8 kJ. D)If the equation is multiplied by 2,ΔH becomes -571.6 kJ. E)For the reaction H₂(g)+ O₂(g)→ H₂O(g),ΔH is not equal to -285.8 kJ.

Question

Quizplus · Accepted Answer

The statement "The value -571.6 kJ pertains to 1 mol of liquid water" is false. The value -571.6 kJ pertains to the formation of 1 mole of liquid water from 2 moles of hydrogen gas and 1 mole of oxygen gas.

Which of the Following Statements Is False Concerning the Reaction