Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below.When 0.015 mol of Na is added to 100.00 g of water,the temperature of the resulting solution rises from 25.00 °C to 31.45 °C.If the specific heat of the solution is 4.18 J $g ^ { - 1 }$ ${ } ^ { \circ } \mathrm { C } ^ { - 1 }$ ,calculate ?H for the reaction,as written.
2Na(s) + 2H₂O(l) ? 2NaOH(aq) + H₂(g) $\Delta _ { \mathrm { r } }$ H= ?

Question

Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below.When 0.015 mol of Na is added to 100.00 g of water,the temperature of the resulting solution rises from 25.00 °C to 31.45 °C.If the specific heat of the solution is 4.18 J

g ^ { - 1 }

{ } ^ { \circ } \mathrm { C } ^ { - 1 }

,calculate ?H for the reaction,as written.
2Na(s) + 2H₂O(l) ? 2NaOH(aq) + H₂(g)

\Delta _ { \mathrm { r } }

H= ?

Quizplus · Accepted Answer

The Answer of Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below.When 0.015 mol of Na is added to 100.00 g of water,the temperature of the resulting solution rises from 25.00 °C to 31.45 °C.If the specific heat of the solution is 4.18 J $g ^ { - 1 }$ ${ } ^ { \circ } \mathrm { C } ^ { - 1 }$ ,calculate ?H for the reaction,as written. 2Na(s)+ 2H₂O(l)? 2NaOH(aq)+ H₂(g) $\Delta _ { \mathrm { r } }$ H= ?

Sodium Metal Reacts with Water to Produce Hydrogen Gas and Sodium