Chem 201 Chapter 8 Worksheet Define the following terms: a) enthalpy - b) internal energy c) state function d) Hess's law e) calorimetry f) thermal equilibrium A
125.6g
piece of gold
(Au)
is submerged in a calorimeter containing
90.0g
of
H_(2)O
, which is initially at
28.0\deg C
. The gold and water reach thermal equilibrium at
36.4\deg C
.
C_(sH2O )=4.184(J)/(g^(**0)C),C_(sAu )=0.129
(J)/(g^(**0)C)
. What is the initial temperature of the gold? Calculate
\Delta H_(rxn)
of the following reactions using the standard enthalpy of formation values below:
Ca(g)\Delta H_(i)^(0)=178.2k(J)/(m)ol,CaO(s)\Delta H_(i)^(0)=-634.9k(J)/(m)ol,H_(2)O(I)\Delta H_(i)^(0)=-285.8kJ,Ca(OH)_(2)(s)\Delta H_(i)^(0)=-985.2
k(J)/(m)ol,SO4(s)\Delta H_(i)^(0)=-296.8k(J)/(m)ol,CaSO_(4)^(**)2H_(2)O(s)\Delta H_(i)^(0)=-2022.63k(J)/(m)ol
. a)
2Ca(g)+O_(2)(g)->2CaO(s)
b)
Ca(s)+2H_(2)O(I)-Ca(OH)_(2)(s)+H_(2)(g)
c)
Ca(s)+SO_(4)(s)+H_(2)O(l)-CaSO_(4)**2H_(2)O(s)
How many grams of
HCl
produced would require
6403kJ
of heat in the reaction below:
3MgCl_(2)(aq)+2H_(3)P(aq)->Mg_(3)P_(2)(s)+6HCl(aq),\Delta H^(0)=157.2k(J)/(m)ol