SDSU Chemistry Heat and Temperature Question

Question 23 pts
What is the energy change when the temperature of 13.6 grams
of solid gold is decreased from 33 °C to 21.2 °C ? Answer with
just the number (no units)
Heat J/g*C
Heat J/g*C
Glass (SiOx) 0.837
Water (1)
Water (s or
Water (g or
Ethanol (1)
Mercury (1)
Question 3
3 pts
A 62.3 g piece of iron at 95.0 °C was immersed into 80.0 g
water at 25.0 °C. The water temperature rose to 30.4 °C.
Calculate the molar heat capacity of the metal.
Answer with just the number (no units)
Answer: ____J/mol*C (number only)
Question 4
3 pts
The following information is given for silver at 1 atm:
boiling point = 2212 °C
A Hvap(2212 °C) = 254 kJ/mol
melting point = 961 °C
A Hfus(961 °C) = 12.0 kJ/mol
specific heat solid= 0.238 J/g°C
specific heat liquid = 0.285 J/g°C
What is AH in kJ for the process of freezing a 32.3 g sample of
liquid silver at its normal melting point of 961 °C. Just need to
give the numerical answer (no units).
Question 5
3 pts
A 42.00 g sample of solid cobalt is initially at 1466.00°C. If the
sample is heated at constant pressure ( = 1 atm), What is the energy
in kJ of heat needed to raise the temperature of the sample
to 1693.00°C. Answer with the number only (no units)
The following information is given for cobalt at 1 atm:
Specific Heat of Fusion
Heat (J/g*C) (KJ/mol)
Heat of
Cobalt (Co)
0.4180 (s)
0.6860 (1)
Mg melting (Temp) 1495.0 °C
Mg vapor. (Temp)
Question 6
3 pts
The following thermochemical equation is for the reaction of iron(III)
oxide(s) with hydrogen(g) to form iron(s) and water(g).
Fe2O3 (s) + 3H2 (g) –> 2 Fe (s) + 3 H2O (g) AH = 98.8 KJ
When 39.6 grams of iron(III) oxide(s) react with excess hydrogen (g)
KJ of energy is
(absorbed or evolved)
3 SF ONLY or the tenth position!
Question 7
4 pts
In an experiment, a 0.3555 g sample
of anthracene (C14H10) is burned completely in a bomb
calorimeter. The calorimeter is surrounded
by 1.080×103 g of water. During the combustion the
temperature increases from 27.72 to 30.41 °C. The
heat capacity of water is 4.184 Jg=10C-1.
The heat capacity of the calorimeter was determined
in a previous experiment to be 935.9 J/°C.
Assuming that no energy is lost to the surroundings,
calculate the molar heat of combustion
of anthracene based on these data.
C14H10(s) + (33/2) O2(g) –
+ Energy
5 H2O(1) + 14 CO2(g)

The molar heat of combustion is [x] KJ (use normal
NOT scientific notation)
Question 8
O pts
Upload your SHOW WORK here as ONE pdf file only for partial credit
(quizzes ONLY).
Must have your name on the top and the questions numbered, I will only
use if you have theses (name and questions numbered) and as a pdf ONLY!
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