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Which of the Following Statements Is False Concerning the Reaction

Question 49

Multiple Choice

Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below?
H2(g) + Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H<sub>2</sub>(g) + O<sub>2</sub>(g) → H<sub>2</sub>O(l) ; ΔH = -285.8 kJ A) Per mole of O<sub>2</sub>,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 H<sub>2</sub>(g) + O<sub>2</sub>(g) → H<sub>2</sub>O(g) ,ΔH is not equal to -285.8 kJ.
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) + Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H<sub>2</sub>(g) + O<sub>2</sub>(g) → H<sub>2</sub>O(l) ; ΔH = -285.8 kJ A) Per mole of O<sub>2</sub>,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 H<sub>2</sub>(g) + O<sub>2</sub>(g) → H<sub>2</sub>O(g) ,ΔH is not equal to -285.8 kJ. O2(g) → H2O(g) ,ΔH is not equal to -285.8 kJ.

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