Answer to Question #96560 in General Chemistry for Taylor

Question

A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 61.9 mL water (where X is a hypothetical metal):

X + 2 H2O → X(OH)2 + H2

In this process, the water temperature rose from 25.0 °C to 36 °C. If 0.00547 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"?

The specific heat of water is 4.184 J g-1 °C-1

Answer 1

Del H = nC_p delT

Del H = change in Emthalpy

Cp= heat capacity

n= no. Of gms

61.9 ml Water = 61.9gm of Water

n = 61.9gm

Del T= 11

Del T =11C

DelH = 61.9*4.184*11