Questions tagged [enthalpy]
A thermodynamic state function describing the total energy content of a system.
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Relation between equilibrium constant and entropy change
Like the Van't Hoff equation, which relates change in enthalpy to equilibrium constant, is there a similar equation for the relation between change in entropy and equilibrium constant?
Consider the ...
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17 views
Need to normalize lattice enthalpy by no. of nearest-neighbor (NN) interactions to equate to NN interaction strength?
I've seen electrostatic interaction energy (from $E\sim \frac{q_1 q_2}{r}$) used to explain differences in lattice enthalpies between different crystalline solids. For example, I've seen it explained ...
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Calculate correct heat output of chemical reaction
A solution with 1 mole $\ce{NaOH}$ is mixed with a solution of 1 mole $\ce{HCl}$ and the total volume is 1 L. The initial temperature is 25 °C. My question is regarding calculating the correct heat ...
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Thermodynamic data related to diazotization reaction
Is there any thermodynamic data available for diazotization of aniline and also for the reduction of the diazonium salt using sodium sulfite? I also want to know the heat of reaction for both the ...
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22 views
Heat And Enthalpy Change [duplicate]
I am studying thermodynamics and I am really confused between enthalpy and heat change . I cannot understand the difference between them.
In Physics we use ∆Q , where as in chemistry we use ∆H . Are ...
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2answers
57 views
Relation between ΔH and ΔE for the reaction in gaseous phase at constant temperature and pressure
Which of the following statements is correct for the reaction at constant temperature and pressure:
$$\ce{CO(g) + \frac{1}{2}O_2(g) -> CO2(g)}$$
$\Delta H = \Delta E$
$\Delta H > \...
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1answer
47 views
Comparing strength of the C-H, N-H, and O-H bonds
$$
\begin{align}
\ce{CH4(g) + Cl(g) &-> CH3(g) + HCl(g)} &\quad ΔH^\circ &= \pu{-14 kJ mol-1}_\mathrm{rxn}\\
\ce{NH4(g) + Cl(g) &-> NH2(g) + HCl(g)} &\quad ΔH^\circ &= \...
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38 views
Trying to understand rationale behind Joule-Thomson experiment
The purpose of the original Joule (as opposed to JT) expansion experiment was to assess intermolecular interactions in real gases. In that experiment, Joule immersed twin glass globes into a water ...
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1answer
36 views
Change in heat of photosynthesis
Consider a plant that uses the energy it receives from the sun to do work (to undergo photosynthesis) to produce glucose. The minimum amount of work this plant can do to produce 1 mole of glucose is ...
1
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1answer
30 views
Heat and work of glucose combustion
$$\ce{C6H12O6(s) + 6 O2(g) -> 6 CO2(g) + 6 H2O(g)}$$
When looking at glucose combustion I found that the change in Gibbs free energy is greater than the change in enthalpy. If we assume the process ...
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1answer
38 views
Is the enthalpy of a molecule determined by the energy of the electrons? [closed]
I understand that the strength of the bond of a molecule is determined by the potential and kinetic energy of the electrons. I also understand that a reaction where the bond strength of the products ...
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19 views
why is white phosphorous given to have ZERO standard heat of formation [duplicate]
why is white phosphorous given to have ZERO standard heat of formation??
while it is well known fact that white phosphorous is highly reactive and is obviously less stable than red and black ...
3
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1answer
192 views
What is meant by electrons moving to lower potential energy?
I am currently learning about chemical bonds in chemistry, and came across somebody who wrote this (source):
"Chemical bonds certainly "contain" potential energy, and the atoms want to move to a ...
4
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1answer
106 views
Would the change in enthalpy (ΔH) for the dissolution of urea in water be positive or negative?
To test the properties of a fertilizer, $15.0\ \mathrm g$ of urea, $\ce{NH2CONH2(s)}$, is dissolved in $150\ \mathrm{mL}$ of water in a simple calorimeter. A temperature change from $20.6\ \mathrm{^\...
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1answer
57 views
Temperature dependency of enthalpy H and entropy S [closed]
In textbooks, I often read that the temperature dependency of the enthalpy of reaction $\Delta_\mathrm{r}H$ and the entropy of reaction $\Delta_\mathrm{r}S$ can be neglected (in a limited $T$-range).
...
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1answer
46 views
Change in Gibbs free energy vs. change in enthalpy
When learning about other thermodynamic quantities, like $\Delta H$, I was taught that this represents the energy absorbed or released by a system after the reaction has gone 100% to completion. For ...
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1answer
83 views
Are precipitations exothermic and/or endothermic?
Should be an easy one. I'm fumbling a concept. I've read precipitations are exothermic. Is this accurate? Why would there be no endothermic precipitation reactions?
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2answers
54 views
Which substances have the highest/lowest enthalpy of formation per gram?
Which substances have the most extreme enthalpies of formation per gram at standard temperature and pressure?
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55 views
Is heating water endothermic?
So I got a problem recently which asked to calculate the amount of energy needed to increase the temperature of 200 g of water from 26 to 51 degrees Celsius. The value I got was 20900 J.
So far I ...
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1answer
50 views
Heat of formation of aqueous H⁺
In my book it is given that by convention heat of formation of aqueous $\ce{H+}$ is taken to be zero. Heat of formation is energy released or absorbed when 1 mole of a compound is formed from its ...
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1answer
32 views
Combining Bond Enthalpies and Enthalpies of Formation
Can I mix formation enthalpies and bond enthalpies in the same calculation?
I think the answer is no, since they are relative measurements, and possibly relative to different things, but I haven't ...
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1answer
53 views
Do endothermic reactions have a higher absolute change in temperature than exothermic reactions? [closed]
or does it depend on the reaction itself. I am conducting an experiment and the endothermic reactions have temperature changes of at least 8 degrees while the exothermic reactions have a change in 1 ...
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24 views
How to describe the enthalpy of acid dissociation in aqueous solutions?
How to describe the enthalpy of acid dissociation in aqueous solutions?
If we had a weak acid "PB" that dissociates to give a proton and a conjugate base. Classically it would be described like the ...
3
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2answers
93 views
Can an exothermic (endothermic) process increase (decrease) internal energy?
We classify exothermic and endothermic processes based on enthalpy change, $\Delta H < 0$ and $\Delta H > 0$ respectively.
I assume this translates to $\Delta U < 0$ and $\Delta U > 0$, ...
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1answer
22 views
Overall enthalpy balance on a mixing process
Let's say I have a mixing process involving $\ce{A}$ and $\ce{B}$ at temperatures $T_\ce{A}$ and $T_\ce{B}$, respectively. The $\ce{AB}$ mix is at temperature $T_p$. Our $ΔH_\mathrm{mix}$ is defined ...
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1answer
38 views
Does enthalpy of dissolution change with temperature?
Dissolution can be either endothermic or exothermic. At higher temperature dissolution is much faster. However, supplying heat also leads to an increase in the internal energy of the system. ...
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1answer
78 views
How does the proticity of an acid affect the enthalpy change of its reaction with a base?
For an experiment I've carried out a series of reactions between monoprotic bases (ammonia and potassium hydroxide) and several acids. Two of these acids were monoprotic (hydrochlori acid and ethanoic ...
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2answers
224 views
Calculating the strength of an ionic bond that contains poly-atomic ions
So the bond association enthalpy for ionic compounds like $\ce{NaCl}$ and $\ce{NaBr}$ can be easily calculated from a Born-Haber cycle. But the way a Born-Haber cycle is constructed it uses info that ...
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22 views
Is there a website or book that contains accepted values for the enthalpy change of the reactions between acids and bases?
I am looking for a website/book/journal/etc. which contains the accepted values for the enthalpy change of the follwoing reactions:
Hydrochloric acid with potassium hydroxide
Hydrochloric acid with ...
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1answer
57 views
What is the difference between ΔfH and H-H° in NIST–JANAF tables?
Can someone explain the difference between $Δ_\mathrm{f}H$ and $H-H^\circ$ in NIST–JANAF tables?
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153 views
What is the molar enthalpy of reaction
When 0.45 g of Zn is added to 50.0 ml of 0.95 M HCl solution, the solution inside the calorimeter heats up by 12 °C. What is the molar enthalpy of the reaction (in kJ/mol)?
I know how to find the ...
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1answer
120 views
Calculating ΔH from bomb calorimetry
Suppose we carry out a reaction in a bomb calorimeter whose starting temperature is $298.15\ \mathrm K$. Here we assume $\Delta V$ is close enough to zero that we consider the process to be at ...
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1answer
51 views
Using Hess's law to find molar enthalpy of formation without an initial reaction [closed]
I'm having issues relating Hess's law to this question:
The given chemical equation represent the combustion of ammonia and the combustion of hydrogen
$$
\begin{align}
\ce{4 NH3 + 3 O2 &-&...
2
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1answer
45 views
How is “the surrounding” and its temperature defined to calculate entropy change during a reaction?
Lets say supercooled liquid water at $263\ \mathrm K$ isobarically changes to solid ice at the same temperature. I wish to calculate the change in entropy of the surroundings and I happen to know the $...
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2answers
78 views
Why enthalpy is defined at a constant pressure?
How absolute enthalpy and enthalpy change are defined? What is the clear difference between enthalpy and heat? Is it the constancy of pressure what makes the enthalpy a state function?
My teacher ...
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1answer
399 views
Explanation of the strength of phosphorus-oxygen bond
When discussing the Wittig reaction, Clayden's Organic Chemistry cites the strength of the $\ce{P=O}$ formed in triphenylphosphine oxide as a driver of the reaction through enthalpy:
The $\ce{P=O}$ ...
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1answer
45 views
Heat of formation method
For enthalpy calculations why is it that in some cases the "heat of formation method" is used? I know that $ΔH_f$ represents the heat required to form the compound at standard temperature and pressure ...
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1answer
85 views
Confusion in change in enthalpy relation
In the equation
$$\Delta H = \Delta U + \Delta PV,$$
under what circumstances can we simplify it into
$$\Delta H = \Delta U + P\,\Delta V + V\,\Delta P$$
by product rule?
In this article (pdf ...
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1answer
152 views
Calculating enthalpy change for a real gas
I know this question would be closed citing it to be a homework question. I posted it earlier also. But believe me I have tried it for myself before and that too many times but then couldn't arrive at ...
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1answer
45 views
How do you calculate the delta H for multiple reactions?
I am having difficulty in a question:
Given that
1. $\ce{N_2(g) \rightarrow 2N(g), \Delta H = 941 kJ/mol}$
2. $\ce{N_2(g) \rightarrow N_2^+ + e^-, \Delta H = 1501 kJ/mol}$
3. $\ce{N(...
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2answers
304 views
When to use internal energy and enthalpy in balances
I am confused as to when you use ΔU and when to use ΔH, I don’t really understand the difference. Is it that ΔU is used for closed systems whilst ΔH is used for open systems?
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Experimental measurement on the ring-strain
for my thesis i calculated the ring-strain of a molecule by MP2 on the computer. I was wondering if there is an easy possibility to get the experimental value of the ring strain. I guess I have to ...
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1answer
124 views
Using thermodynamics to predict the acid-base character of fluoride ion in water
I was working through the end-of-chapter exercises of the acid-base chapter in Shriver's Inorganic Chemistry when I came across the following problem:
4.7. The effective proton affinity $\ce{A^{'}_{...
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1answer
136 views
What is the molar enthalpy? [closed]
In a practice test there's the question, 'Given that the combustion of.305g of glucose causes a raise of temperature of 6.30C of a caloromiter with total heat capacity C=755J/C and the molecular ...
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1answer
62 views
How can there be an enthalpy of formation for gaseous water?
Under standard conditions( 1 bar and 298.15 K), water will be in the liquid state. So how can you find the enthalpy of formation for gaseous water at standard conditions(as found in the back of all ...
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1answer
140 views
Why do we use pV term independent of U in the equation H = U + pV? [duplicate]
I have read the following definition of enthalpy in my textbook:
A substance has to occupy some space in its surroundings depending upon its volume ($V$). It does against the compressing influence ...
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1answer
71 views
thermochemistry problem confusion
I can understand upto where the ideal gas equation is used to calculate volume of steam. But on trying to find out $ \Delta V$ , i saw that there are no gases on the reactant side so then $P\Delta V=(\...
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1answer
254 views
Insoluble salts and Gibbs free energy
Is it true that according to gibbs free energy equation, insoluble salts such as AgCl don't dissolve because the process would be too endothermic? The right side of the equation, TΔS, would have to be ...
4
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1answer
372 views
How to calculate the enthalpy of reaction using Gaussian 09?
I'm having a hard time trying to understand what's the correct way to calculate the enthalpy of reaction given that I've already calculated the frequencies of my compounds in Gaussian. Below I show ...
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189 views
How to calculate the enthalpy of fusion at a different temperature?
The heat capacity of liquid iodine is $80.7$ $\ce{J*K^{-1}*mol^{-1}}$, and its enthalpy of vaporization is $41.96$ kJ $\ce{*mol^{-1}}$ at its boiling point ($184.3$ $\ce{^oC}$). Furthermore, the ...
