# 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)
Substance
Specific
Heat J/g*C
Specific
Substance
Heat J/g*C
Glass (SiOx) 0.837
Water (1)
4.186
2.090
Silicon
0.703
Water (s or
ice)
Water (g or
steam)
2.010
Calcium
0.640
Ethanol (1)
2.400
Chromium
0.461
Beryllium
1.830
Copper
0.387
Wood
1.700
Brass
0.380
1.230
Silver
0.234
Magnesium
Aluminum
Marble
0.897
Mercury (1)
0.140
0.860
Gold
0.129
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)
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:
Compound
Specific Heat of Fusion
Heat (J/g*C) (KJ/mol)
Heat of
Vaporization
(KJ/mol)
Cobalt (Co)
0.4180 (s)
16.91
376.5
0.6860 (1)
Mg melting (Temp) 1495.0 °C
Mg vapor. (Temp)
3097.0°C
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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