Hydrogen Peroxide Decomposes to Water and Oxygen at Constant Pressure $2 \mathrm { H } _ { 2 }$

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: $2 \mathrm { H } _ { 2 }$ $\mathrm { O } _ { 2 }$ (l) ? $2 \mathrm { H } _ { 2 }$ O(l) + $\mathrm { O } _ { 2 }$ (g) $\Delta _ { \mathrm { r } }$ H = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

A) -0.0217 kJ $\mathrm { mol } ^ { - 1 }$
B) 1.44 kJ $\mathrm { mol } ^ { - 1 }$
C) -2.31 × 10⁴kJ $\mathrm { mol } ^ { - 1 }$
D) -23.1 kJ $\mathrm { mol } ^ { - 1 }$
E) -11.5 kJ $\mathrm { mol } ^ { - 1 }$

Correct Answer:

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