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Thermochemistry
Page 2
Questions (383)
How much methane, in grams, must be burned to release 542 kJ of heat? H=-802kJ
4 answers
asked by
Luke
3,115 views
Hi, could someone please take a look at the following question?
Use the data given below to construct a Born-Haber cycle to
4 answers
asked by
Constantine
7,829 views
Hydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the following reaction.
CH4(g) + NH3(g) → HCN(g)
4 answers
asked by
Emily
3,948 views
3. If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mL of a 1.5M NaOH
solution at 21.50C that is in a calorimeter,
3 answers
asked by
Meredith
1,342 views
The heat of neutralization of HCl(aq) and NaOH(aq) is -55.90 kJ/mol of water produced. If 50.00 mL of 1.16 M NaOH at 25.15 ºC
3 answers
asked by
Alexis
1,165 views
Octane (C8H18) undergoes combustion according to the following thermochemical equation:
2 C8H18(l) + 25 O2(g) ---> 16 CO2(g) + 18
4 answers
asked by
Robert
4,884 views
At 25°C the following heats of reaction are known:
2C2H2 + 5O2 ---> 4CO2 + 2H2O; ΔH = -2600 kJ C + O2 ---> CO2 ; ΔH = -394 kJ
4 answers
asked by
Kaitie
3,551 views
Calculate the enthalpy change (ΔH) for: HCl(aq) + NH3(aq) → NH4Cl(aq)
The reaction of 50.0 mL of 1.00 M HCl with 50.0 mL of
4 answers
asked by
Jim
5,725 views
Hydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the following reaction.
CH4(g) + NH3(g) → HCN(g)
3 answers
asked by
caroline
686 views
Complete the Hess’ cycle using the values given in the table and hence calculate the enthalpy
change, ∆Hr , for this
4 answers
asked by
hiba
546 views
In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of 0.660 M HCl. The reaction caused the
4 answers
asked by
Heather
830 views
Butane, C4H10, is widely used as a fuel for disposable lighters. When one mole of butane is burned in oxygen, carbon dioxide and
3 answers
asked by
Chris
2,558 views
Calculate the value (calories) for the heat of solution.
Mass of NaOH: 2.03 g ΔT for reaction A : 8 °C
4 answers
asked by
Maria
1,606 views
Select the two conditions that must be met by a thermochemical equation so that its standard enthalpy change can be written as
4 answers
asked by
write2khin
2,494 views
Can anyone help me with these Chemistry questions? I am trying to study for an upcoming test and its just not sinking in as well
4 answers
asked by
Dina
1,241 views
Thermochemistry:
1. Calculate the amount of heat required to decompose 3.5 moles of sodium bicarbonate. 2NaHCO3 + 129 kJ
4 answers
asked by
Bethany
2,877 views
Consider the following reaction:
2H2 (g) + O2 (g) 2H2O (l) ΔH = -572 kJ a. How much heat is evolved for the production of
4 answers
asked by
Anonymous
3,880 views
Calculate ΔG° (in kJ/mol) for the following reaction at 1 atm and 25 °C:
C2H6 (g) + O2 (g) → CO2 (g) + H2O (l) (unbalanced)
4 answers
asked by
holly
2,481 views
You can mix 100.mL of 1.0 M HCl with 100 mL of 1.0 NaOH, both at 25 degree Celcius. The temperature of your calorimeter rises by
4 answers
asked by
Sanaya
3,320 views
81) According to the following thermochemical equation, what mass of HF (in g) must react in order to
produce 345 kJ of energy?
4 answers
asked by
sean
5,292 views
The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts
4 answers
asked by
tank
2,289 views
How much energy is required to decompose 765 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol
4 answers
asked by
yr
5,439 views
Find DHo for BaCO3(s) --> BaO(s) + CO2(g) given
2 Ba(s) + O2(g) --> 2 BaO(s) DHo = -1107.0 kJ Ba(s) + CO2(g) + 1/2 O2(g) -->
5 answers
asked by
harsha
2,829 views
1. The thermochemical equation for the production of nitrogen monoxide is N2 (g) + O2 (g) ↔ 2NO (g) – 180.9 kJ. The heat of
4 answers
asked by
Rajeshwari
1,612 views
a sample of an ionic compound is dissolved in water and the water gets colder. what is acting as the system?what is acting as
4 answers
asked by
Anonymous
1,346 views
I don't know why it was marked wrong. This is what it said: Where is the 5.64 coming from? Is this a typo?(thank you)
HINT To
4 answers
asked by
patrick
1,945 views
How much heat is needed to produce 10.5 moles of methane gas
4 answers
asked by
Lan
1,232 views
In a constant-pressure calorimeter, 65.0 mL of 0.330 M Ba(OH)2 was added to 65.0 mL of 0.660 M HCl. The reaction caused the
4 answers
asked by
Emily
637 views
Consider the reaction
2 Al2O3(s) → 4 Al(s) + 3 O2(g). ∆H = +3339.6 kJ/mol What is the change in heat when 0.455 L of a 3.60 M
2 answers
asked by
Anonymous
1,243 views
The enthalpy of combustion of butane C4H10 is described by the reaction:
C4H10(g) + (13/2) O2(g) -> 4CO2(g) + 5H2O(g) ΔH°rxn =
3 answers
asked by
anon
5,754 views
A 1.55-g sample of propane, C3H8, was burned in a bomb calorimeter whose total heat capacity is 12.3 kJ/°C. The temperature of
4 answers
asked by
Nisah
1,142 views
The enthalpy formation of ethanol, C2H5OH, is -277.0 kJ/mol @ 298.15 K. Calculate the enthalpy of combustion of one mole of
4 answers
asked by
Morgan
2,822 views
Calculate Delta H for 4NH3 + 5O2 --> 4NO + 6H2O
using: N2 +O2 --> 2NO DH= -180.5 kJ N2 + 3H2 --> 2NH3 DH= -91.8 kJ 2H2 + O2 -->
4 answers
asked by
Taylor
10,720 views
N2H4(g) + H2(g)--> 2 NH3(g) H1 = –1876kJ
3 H2(g) + N2(g)--> 2 NH3(g) H2 = –922 kJ The H.f for the formation of hydrazine: 2
4 answers
asked by
CHem
4,215 views
When 1.07E-1 g of Zn(s) combines with 5.64E1 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases
3 answers
asked by
Tej
755 views
Calculate the change in enthalpy when 52.0 g of solid chromium at 25°C and 1 atm pressure is oxidized. (H°f for Cr2O3(s) is
3 answers
asked by
Jessica
2,713 views
One reaction of iron with hydrochloric acid is represented by the following
thermochemical equation. Fe(s) + 2HCl(aq) ? FeCl2(aq)
3 answers
asked by
Raul
2,049 views
When a 0.432g sample of a mixture of volatile hydrocarbons is burned in a bomb calorimeter with heat capacity of 3046 J/C, the
3 answers
asked by
Ashley
5,047 views
Use the equations with the enthalpy information given below to calculate the ÄH° for the reaction:
S(s) + O2(g) --> SO2(g) S(s)
4 answers
asked by
Anonymous
1,683 views
The enthalpy of neutralization for the reaction of a strong acid with a strong base is -56 kJ/mol of water produced. How much
4 answers
asked by
Bill
1,468 views
Consider the reaction:
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH = - 890.3 kJ What volume of CH4(g) at 25°C and 755 Torr will
3 answers
asked by
Kamila
781 views
The heat of reaction for burning 1 mole of a certain compound X is known to be -477.7 kJ. The calorimeter constant of the bomb
4 answers
asked by
Jacob
1,174 views
What is the standard heat of reaction (H0) for the combustion of ethane, C2H6(g), to form carbon dioxide gas and water?
2C2H6(
4 answers
asked by
thisfoolneedshelp
2,177 views
Many portable gas heaters and grills use propane, C3H8(g), as a fuel. Using standard enthalpies of formation, calculate the
3 answers
asked by
Samantha
606 views
calculate enthalpy of H for the reaction
N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) +
4 answers
asked by
Rose Bud
3,578 views
When 2.53 g of NaOH(s)(40.0g/mol) dissolves in 100.0 g of water, the temperature of the solution changes from 20 degrees C to
4 answers
asked by
Tara
558 views
I have to find the molar enthalpy of combustion of pentane. I have this info:
5C(s) + 6H2 >>> C5H12 Hf= -173.5kJ C+O2>>> CO2 Hf=
3 answers
asked by
Hey!
1,859 views
Consider the following reaction:
2CH3OH(g)→2CH4(g)+O2(g),ΔH=+252.8 kJ 1. Calculate the amount of heat transferred when 28.0 g
1 answer
asked by
rhea
398 views
5 grams of C2H5OH is burned in a bomb calorimeter, producing dqv = -148.3 kJ, by the
following reaction: C2H5OH(l) + 3O2(g) 6
3 answers
asked by
Muneeb
195 views
A dilute aqueous solution with a mass of 43.8031 g has a temperature increase of 10.2 ^\circ
∘ C. Calculate the enthalpy change
3 answers
asked by
Anonymous
501 views
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Parent Categories (9)
Acids and Bases
Chemical Reactions
Chemistry
Chemistry Knowledge
Physical Chemistry
Physics
Reactions and Energy
Stoichiometry
Thermodynamics