Calculating Heat Produced in a Chemical Reaction

  • Thread starter Thread starter JoeMann
  • Start date Start date
  • Tags Tags
    Joules
AI Thread Summary
To calculate the heat produced in the reaction, first determine the number of moles of Cl2 produced, which is given as 0.0100 mol. The reaction's enthalpy change (ΔrH) is -202 kJ per mole of Cl2 formed. Multiply the moles of Cl2 by the enthalpy change to find the total heat produced, resulting in q(system) = 0.0100 mol * -202 kJ/mol = -2.02 kJ, or -2020 J. The temperature change is not necessary for this calculation since the heat produced is directly derived from the reaction's enthalpy. Thus, the heat produced in the system is -2020 J.
JoeMann
Messages
1
Reaction score
0

Homework Statement


OCl–(aq) + Cl–(aq) + 2H+(aq) Cl2(aq) + H2O ΔrH = -202 kJ mol–1
25.0mL of a solution 0.400mol L–1 in both OCl– and Cl– was reacted with excess hydrochloric acid. The mass of the solution after mixing was 100 g.
n(reaction) = 0.0100 mol

Find q(system) in joules.
Assume that the temperature change of the vessel in which the experiment is carried out is negligible
Assume that the heat capacity of the mixture is the same as the specific heat capacity of water (4.184 J g–1 K–1).

Homework Equations

I know somewhere you have to use the formula q = mcΔT but I am unsure what to do because there is no temperature in the question.

The Attempt at a Solution



I have tried multiplying the mass and temp change but I think i am wrong. Please help?
 
Physics news on Phys.org
It is not about q = mcΔT.

You are told how much heat is produced per mole of produced Cl2. How many moles were produced?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
View full post »

Thread 'Prove that evolution is constant (Provide at least two arguments to support your position)'

I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
View full post »

Similar threads

Calculating Delta-H for a Reaction using a Coffee-Cup Calorimeter Method
Replies
3
Views
4K
Chemistry How do we interpret the steps in the algorithm to balance a redox equation?
Replies
7
Views
2K
Chemistry How to find the pH of a galvanic cell (MIT OCW problem set)
Replies
2
Views
3K
Calculate the final temperature of the solution
Replies
5
Views
3K
What Is the Final Temperature of a Squeezed Hot Pack with LiCl and Water?
Replies
7
Views
2K
Chemistry Understanding Heat of Neutralization in Acid-Base Reactions
Replies
9
Views
3K
Chemistry Understanding the calculation of enthalpy of the formation of benzene
Replies
3
Views
2K
Why is activity of solvated components equal to 1?
Replies
1
Views
2K
How to calculate heat from enthelpy of reaction
Replies
5
Views
2K
Does sodium bicarbonate solution release CO2 when heated?
Replies
2
Views
4K

Hot Threads

Recent Insights

Back
Top