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Thermochemistry
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Questions (383)
Hi there, I need some help with my homework problem for chemistry, What is the balanced thermochemical equation for glucose
1 answer
asked by
Shylo
355 views
A balanced chemical reaction that includes the heat change (evolved or absorbed △H) during the reaction is called the
8 answers
asked anonymously
47 views
5.50 g of sodium hydroxide is dissolved in 175 mL of water. Using a coffee-cup calorimeter, the temperature change of the water
7 answers
asked anonymously
52 views
Calculate the change in heat:
2 Na(s) + 2 H2O(l) > 2 NaOH(aq) + H2(g) So far this is what I have: 2 H20 --> 2 H2 + O2 2(285.83)
1 answer
asked by
Jayd
1,037 views
Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous
1 answer
asked by
Jon
661 views
The standard molar enthalpies of formation of H2O(l) are given as:
H2(g) + 1/2 O2(g) → H2O(l) △f Ho = –285.8 kJ/mol What
4 answers
asked anonymously
52 views
M grams of sucrose give enthalpy change of △H kJ/mol on combustion. What is the effect on enthalpy change when the mass of the
6 answers
asked anonymously
56 views
Given:
*Fe2O3(s)+3CO(s)-->2Fe(s)+3CO2(g)(delta h is -23kJ) *3Fe2O3(s)+CO(g)-->2Fe3O4(s)+CO2(g)(delta h is -39kJ)
6 answers
asked by
tanisha
3,021 views
In a thermochemistry experiment the reaction of 0.0857 g of an unknown metal and an excess of 4.0 M HCl resulted in a 0.210 mL
6 answers
asked by
Raj
2,848 views
Given H2(g) + (1/2)O2(g) ---> H2O(l), dH = -286 kJ/mol, determine the standard enthalpy change for the reaction 2h2O(l) --->
3 answers
asked by
AJ
2,713 views
The combustion of methane in a laboratory burner is represented by the following equation:
CH4 + 2 O2 > CO2 + 2 H2O Given the
6 answers
asked by
Mike
2,133 views
Find the false statement(s) about the thermochemistry experiment in which nitric acid is reacted with sodium hydroxide, and the
3 answers
asked by
Anonymous
1,883 views
2. Baking soda is sodium bicarbonate (NaHCO3). When you heat baking soda, it breaks down into sodium carbonate powder (Na2CO3),
3 answers
asked by
dd
1,825 views
Baking soda is sodium bicarbonate (NaHCO3). When you heat baking soda, it breaks down into sodium carbonate powder (Na2CO3),
4 answers
asked by
student
1,707 views
Give delta H for the combustion of propane: C3H8+5O2+3CO2+4H20 +530KCAL
delta h= -530 KCAL But how do i figure out how to get
3 answers
asked by
ashley
1,555 views
Nitric acid, HNO3, was first prepared 1200 years ago by heating naturally occurring sodium nitrate (called saltpeter) with
3 answers
asked by
shahreen
1,472 views
Which of the following statements is incorrect concerning the thermochemical equation below?
2SO3(g) 2SO2(g) + O2(g); H°
3 answers
asked by
Jessica
1,447 views
If 15.0 kJ are released when 1.40 g of F2 reacts with an excess of SiH4, complete the thermochemical equation below.
SiH4(g) + 2
4 answers
asked by
Rach
1,450 views
Construct a Born Haber cycle for the formation of calcium oxide showing clearly using equations, the steps of the enthalpy
3 answers
asked by
Demario
1,386 views
When 10.0 g of ammonium nitrate (molar mass= 80 g/mol) are dissolved in 1.00 L of water in a bomb calorimeter with a heat
2 answers
asked by
Sam
1,359 views
The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H
4 answers
asked by
Kristin
1,326 views
Calculate the change in enthalpy produced by dissolving 14.3 g of NaOH in 65.0 g of water if the temperature increases 49.1°C
2 answers
asked by
Morgan
1,291 views
If 8.00 g of ammonuim nitrate is dissolved in 1000 ml of water for use as a plant fertilizer, the water decreases in temperature
2 answers
asked by
Nicole
1,286 views
Use enthalpies of formation from the textbook to calculate the standard enthalpy of the reaction for the following methane-
2 answers
asked by
Kay
1,253 views
N2H4 reacts with oxygen to yield nitrogen gas and water . The reaction of 3.80g n2h4 evolves 73.7kj of heat. what's the enthalpy
3 answers
asked by
olexandra
1,251 views
The enthalpy change for the solution process when solid sodium hydroxide dissolves in water is -44.4 kJ/mol. When a 13.6 g
2 answers
asked by
Anonymous
1,243 views
N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = –264 kJ/mol ΔS° = –278 J/(mol∙K)
a. Using the information provided above (only),
1 answer
asked by
chamy
1,209 views
Ca(OH)2(s) −→ CaO(s) + H2O(g)
Given: Ca(OH)2(s) −→ Ca(s) + O2(g) + H2(g) ∆H = 973.3 kJ/mol 2 Ca(s) + O2(g) −→ 2
2 answers
asked by
jane
1,156 views
How much heat (in Joules) is gained by the water when a chemical reaction takes place in 100.0 ml aqueous solution, has a
2 answers
asked by
shelle
1,151 views
Calculate Hrxn for the reaction below.
2 NOCl(g) N2(g) + O2(g) + Cl2(g) You are given the following set of reactions. 1/2 N2(g) +
2 answers
asked by
mara
1,149 views
Which of the following statements is incorrect concerning the thermochemical equation below?
2SO3(g) 2SO2(g) + O2(g); H°
1 answer
asked by
Kayla
1,130 views
If the standard enthalpy of formation of PH3(g) is +5.4 kJ mol-1, calculate the reaction enthalpy for
2PH3(g)--->2P(s)+3H2(g)
2 answers
asked by
Sam
1,129 views
Given the thermochemical equation:
2ZnS(s) + 3O2(g) „³ 2ZnO(s) + 2SO2(g) £GH = --879 kJ Calculate the heat evolved (in kJ)
3 answers
asked by
Shayla
1,143 views
In a coffee-cup calorimeter, 1.50 g of NH4NO3 is mixed with 72.0 g of water at an initial temperature of 25.00°C. After
3 answers
asked by
Courtney
1,132 views
A calorimeter contains 30.0 mL of water at 11.0 degrees C. When 1.50 g of X (a substance with a molar mass of 65.0 g/mol) is
2 answers
asked by
Abby
1,129 views
The combustion of benzoic acid releases 26.38kJ/g and is often used to calibrate a bomb calorimete. The combustion of 1.045g of
10 answers
asked by
Sindy
1,122 views
The value of ƒ¢H�‹ for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of
2 answers
asked by
Harlem
1,090 views
Given the Data:
N2(g) + O2g) = 2NO(g) delta H = 180.7kj, 2NO(g) + O2(g) = 2NO2(g) delta H = 0113.1kj, 2N2O(g) = 1N2(g) + O2(g)
2 answers
asked by
Dan
1,122 views
If 16.9 kJ are released when 1.50 g of O2 reacts with an excess of NO, complete the thermochemical equation below.
4 NO(g) + 3
3 answers
asked by
Tiffany
1,096 views
How much heat is released when a mixture containing 10.0g CS2 and 10.0 g Cl2 reacts by the equation.
CS2 + 3Cl2 ----> S2Cl2 +
4 answers
asked by
Lauren
1,087 views
In a constant-pressure calorimeter, 50.0 mL of 0.300 M Ba(OH)2 was added to 50.0 mL of 0.600 M HCl. The reaction caused the
7 answers
asked by
Eric
1,080 views
The main component of nail polish remover is acetone, which has ∆Hvap= +31.3 kJ/mol. How many kJ of energy will be exchanged
3 answers
asked by
anonymous
1,067 views
DeltaH and DeltaU are nearly the same in all the following processes except
a.F2(g)+H2(g) --> 2HF(g) b.3O2(g) --> 2O3(g) c.CuO(s)
2 answers
asked by
jessica
1,063 views
When coal is mined, it is tested for how much heat it can produce when it burns. A 1.245g sample of coal was placed into a
3 answers
asked by
A. Pool
1,026 views
Hydrogen peroxide decomposes according to the following thermochemical reaction
H2O2 --> H2O +1/2 O2 ; H= -98.2 kJ calculate the
3 answers
asked by
Brittany
1,041 views
2C6H6(l) + 15O2(g) -> 12CO2(g) + 6H2O(l) + 6542 kJ
If the heat from burning 7.000 g of C6H6 is added to 5691 g of water at 21
4 answers
asked by
David
1,034 views
7. (a) Determine the crystal lattice energy for LiF(s) given that the ∆Hsubl for Li = 155kJ/mol,
∆H0f for F(g) = 78.99kJ/mol,
2 answers
asked by
ceasar4
1,009 views
The enthalpy of cimbustion for Octane vapor, C8H18, a component of gasoline, is -5512.0kJ/mol.
a. Write the equation for the
1 answer
asked by
cool
1,011 views
Given the data below, calculate the total heat (in J) needed to convert 20.0 g of liquid ethanol (C2H5OH) at 40.0 oC to gaseous
2 answers
asked by
Alex
982 views
Calculate the standard free-energy change for the following reaction at 25 °C. Standard reduction potentials can be found here.
1 answer
asked by
Kate
981 views
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Parent Categories (9)
Acids and Bases
Chemical Reactions
Chemistry
Chemistry Knowledge
Physical Chemistry
Physics
Reactions and Energy
Stoichiometry
Thermodynamics