Give the thermochemical equation for the formation of ammonium nitrate (AHF = -365.6 kJ/mol). What is...

Question

Question

Give the thermochemical equation for the formation of ammonium nitrate (AHF = -365.6 kJ/mol). What is the enthalpy of formati

Answer 1

Answer #1

In equation of formation, only elements are present as Reactants. Thermochemical equation is :

N ₂(g) + 2H ₂(g) + 3/2 O ₂(g) -> NH ₄NO₃(s)

Enthalpy of formation of Reactants is zero.

Answer 2

Similar Homework Help Questions

- The standard enthalpy of formation, AH, of N2O3(g) is 91.2 kJ/mol. Write the thermochemical equation...

- The standard enthalpy of formation, AH, of N2O3(g) is 91.2 kJ/mol. Write the thermochemical equation corresponding to this.
5. Calculate the enthalpy of dissolution for ammonium nitrate in water in kJ/mol. Lattice energy the...

5. Calculate the enthalpy of dissolution for ammonium nitrate in water in kJ/mol. Lattice energy the At step, + Alt step, + A H stepe + AH" step, + AH steps a = mx CS AT =110.07(4.184 1(-6.80 9 242,672 J 1 2 86.2 KT ! Data Collection Record your data in an organized manner. See the Data Sheet for Lab 7 as an example. 'he better your ex mass of H2O=139.5lg 40.9sq = 98.56 an ass NHU O: 10g...
The change in enthalpy for dissolving ammonium nitrate in water is 26 kJ/mol. Determine the amount...

The change in enthalpy for dissolving ammonium nitrate in water is 26 kJ/mol. Determine the amount of ammonium nitrate (in grams) that was dissolved in water to make 50.0 mL of solution if the temperature of a coffee cup calorimeter changes from 25.3°C to 21.5°C. Assume the density of the solution is 1.0 g/mL and the heat capacity of the solution is 4.2 J/g°C.

What is the standard enthalpy of formation (AHf) in kJ of NO2(g) given: 2 NO28) →N2(g)...

What is the standard enthalpy of formation (AHf) in kJ of NO2(g) given: 2 NO28) →N2(g) + 202(g) AHrxn = -67.6 kJ
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and...

The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
2. A cold pack consists of an inner pouch containing ammonium nitrate, NHĄNO (), and an...

2. A cold pack consists of an inner pouch containing ammonium nitrate, NHĄNO (), and an outer pouch of water. Twisting the pack breaks the inner pouch and allows the water and ammonium nitrate to mix. As the ammonium nitrate dissolves, the temperature of the surroundings decreases. The energy change per mole of ammonium nitrate dissociated is 25.7 kJ. (a) Classify the reaction as endothermic or exothermic. [ans: endothermic (b) Draw a potential energy diagram for the reaction. Label the...

Write the thermochemical equation for each of the following. Be sure to give the physical state...

Write the thermochemical equation for each of the following. Be sure to give the physical state for all reactants and products in the chemical equation and use the appropriate, complete symbol for the enthalpy change, including units. a. The standard enthalpy of formation of water. b. The standard bond dissociation enthalpy for H2 at 298K. c. The standard enthalpy of combustion of liquid methanol. 3. What do we mean by the reference state? 4. Why is the standard enthalpy of...
Given the thermochemical equation: 2A B AH = -41.6 kJ/mol, what is AH for the following...

Given the thermochemical equation: 2A B AH = -41.6 kJ/mol, what is AH for the following reaction: 3B + 6A O 41.6 kJ/mol O-124.8 kJ/mol 124.8 kJ/mol -41.6 kJ/mol
The standard enthalpy of formation of NaF(s) is -573.6 kJ/mol, and the standard enthalpy of formation of NaF(aq, 1m) is -572.8 kJ/mol. Determine the standard enthalpy of solution of NaF. -0.8 kJ/mol -572.0 kJ/mol +0.8 kJ/mol -1146.4 kJ/mol +1146.4 kJ

The standard enthalpy of formation of NaF(s) is -573.6 kJ/mol, and the standard enthalpy of formation of NaF(aq, 1m) is -572.8 kJ/mol. Determine the standard enthalpy of solution of NaF.-0.8 kJ/mol-572.0 kJ/mol+0.8 kJ/mol-1146.4 kJ/mol+1146.4 kJ/mol

Question 3 1 pts The heat of solution of ammonium nitrate is 26.2 kJ/mol. When ammonium...

Question 3 1 pts The heat of solution of ammonium nitrate is 26.2 kJ/mol. When ammonium nitrate solid is dissolved in water at room temperature the beaker containing the solution will start out getting colder, but will soon get very hot will likely feel warm to the touch will likely feel cold to the touch will need to be large enough to hold the extra heat. No transfer to heat