Question
In: Chemistry
Sulfur (2.56 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased...
Sulfur (2.56 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased from 21.25 °C to 26.72 °C. The bomb has a heat capacity of 923 J/K, and the calorimeter contained 815 g of water. Calculate ΔU per mole of SO2 formed for the reaction
S8(s) + 8 O2(g) → 8 SO2(g)
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Pure sulfur is burned with 63% excess air according to the following reaction. S + O2...
Pure sulfur is burned with 63% excess air according to the
following reaction.
S + O2 = SO2 The furnace gases formed enter a reactor under a
pressure of 1 atm at 500 ° C.
80% of SO2 is converted into SO3 by SO2 +1/2 O2 =SO3 reaction.
According to this,
a) Calculate the equilibrium constant Kp of the SO2 +1/2 O2 = SO3
reaction. (10 points)
b) What should be the reactor pressure to increase the conversion
rate of...
Calculate the theoretical flame temperature for CO gas burned at constant pressure with 100% excess air,...
Calculate the theoretical flame temperature for CO gas burned
at constant pressure with 100% excess air, when the reactants enter
at 100°C.
Please show work, do not copy the
solution founded. show your solution! if you can not answer this
question, then do not attempt to copy others' work.
In an adiabatic, constant-volume bomb calorimeter, a combustion of 0.7362g of naphthalene (C10H8) caused the temperature...
In an adiabatic, constant-volume bomb calorimeter, a combustion
of 0.7362g of naphthalene (C10H8) caused the temperature to rise of
5.707 Celcius. The final temperature was 298.000K. The heat
capacity of the calorimeter, Ccal was 10290 J/K . (Note: this value
of Ccal includes the contribution from water.) The molar enthalpies
of formation of CO2(g) and H2O(l) are: -393.522 kJ/mol, -285.830
kJ/mol, respectively Mm(C)= 12.01 g/mol and Mm(H)= 1.001 g/mol.
a.) Calculate deltaUc , deltaUcm , delta Hcm for this combustion...
In the (Bomb Calorimetry) experiment, 1.10 g of anthracene (C14H10) was burned in a constant volume...
In the (Bomb Calorimetry)
experiment, 1.10 g of anthracene (C14H10) was
burned in a constant volume bomb calorimeter. The temperature of
water rose from 20.28 °C to 24.05 °C. If the heat capacity of the
bomb plus water was 10.17 kJ/°C: In the
(Bomb Calorimetry) experiment, 1.10 g of
anthracene (C14H10) was burned in a constant
volume bomb calorimeter. The temperature of water rose from 20.28
°C to 24.05 °C. If the heat capacity of the bomb plus water was...
A sample of K(s) of mass 2.720 g undergoes combustion in a constant volume calorimeter at...
A sample of K(s) of mass 2.720 g undergoes combustion in a
constant volume calorimeter at 298.15 K. The calorimeter constant
is 1849 JK−1, and the measured temperature rise in the inner water
bath containing 1439 g of water is 1.60 K.
a) Calculate ΔU∘f for K2O.
b) Calculate ΔH∘f for K2O.
the answer for ΔU∘f = -362 kJ⋅mol−1
and for ΔH∘f =
-363 kJ⋅mol−1
how they got that answers ????
Part 1: A 1.07 g sample of caffeine (C8H10N4O2) burns in a constant-volume calorimeter that has...
Part 1: A 1.07 g sample of caffeine (C8H10N4O2) burns in a
constant-volume calorimeter that has a heat capacity of 7.28 kJ/K.
The temperature increases from 297.65 K to 301.38 K. Determine the
heat (qv) associated with this reaction.
Part 2:Now use the data above to find ΔE for the combustion of
one mole of caffeine
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A bomb calorimeter, or constant volume calorimeter, is a device
often used to determine the heat of combustion of fuels and the
energy content of foods. Since the "bomb" itself can absorb energy,
a separate experiment is needed to determine the heat capacity of
the calorimeter. This is known as calibrating the calorimeter. In
the laboratory a student burns a 0.466-g sample of 1,8-octanediol
(C8H18O2) in a bomb calorimeter containing 1200. g of water. The
temperature increases from 25.90 °C...
1.A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the...
1.A bomb calorimeter, or a constant volume calorimeter, is a
device often used to determine the heat of combustion of fuels and
the energy content of foods. In an experiment, a 0.3807 g sample of
1,6-hexanediol (C6H14O2) is burned completely in a bomb
calorimeter. The calorimeter is surrounded by 1.139×103 g of water.
During the combustion the temperature increases from 25.30 to 27.59
°C. The heat capacity of water is 4.184 J g-1°C-1. The heat
capacity of the calorimeter was...
A)A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A)A bomb calorimeter, or constant
volume calorimeter, is a device often used to determine the heat of
combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is
needed to determine the heat capacity of the calorimeter. This is
known as calibrating the
calorimeter.
In the laboratory a student burns a 0.392-g sample
of bisphenol A
(C15H16O2) in a
bomb calorimeter containing 1140. g of water. The
temperature increases from 25.00...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A bomb calorimeter, or constant volume calorimeter, is a device
often used to determine the heat of combustion of fuels and the
energy content of foods. Since the "bomb" itself can absorb energy,
a separate experiment is needed to determine the heat capacity of
the calorimeter. This is known as calibrating the calorimeter. In
the laboratory a student burns a 0.337-g sample of bisphenol A
(C15H16O2) in a bomb calorimeter containing 1040. g of water. The
temperature increases from 25.90...
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