How Does Doubling Zinc Mass Affect Temperature Change in ZnO Formation?

In summary, the study investigates the impact of doubling the mass of zinc on the temperature change during the formation of zinc oxide (ZnO). It explores the relationship between the increased zinc mass and the resulting thermal effects, providing insights into the thermodynamic processes involved in ZnO synthesis. The findings suggest that greater zinc mass leads to more significant temperature changes, which could have implications for optimizing ZnO production in various industrial applications.
  • #1
cutielollipop
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Homework Statement
I'm having trouble understanding whether q stays constant? If it does, then for part b) does q stay the same?
Relevant Equations
q = mcdeltaT
Experiment equation: Zn(s) + 2HCL(aq) -> 2ZnCl(aq) + H2(g)

a) If the the mass of zinc solid used was doubled, what effect would this have on temperature change?

Answer: if mass of zinc increases, there will be an increase in zinc particles which increases the collisions between particles and increases the average kinetic energy therefore giving higher temperature change

b) What would have been the number of joules evolved (q)?

c)What effect would this have on delta H?
delta H would increase by a factor of 2 since the mass is doubled, so the number of mols has also doubled.
 
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  • #2
Question is a bit poorly worded or you posted it incomplete, as the answer depends on several other factors - mainly on what is the limiting reagent in the setup.

Amount of heat produced is directly proportional to the amount of zinc that reacted.

Q is not much different from ΔH in that regard (see your answer to c.) - assuming there was a sufficient excess of acid.
 
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  • #3
Thx for your reply. I have figured out the answer as I realized that zinc was the limiting reagant.
 
  • #4
Yes, q is an extensive property.
 

FAQ: How Does Doubling Zinc Mass Affect Temperature Change in ZnO Formation?

What is the enthalpy of formation of ZnO?

The enthalpy of formation of ZnO is the change in enthalpy when one mole of zinc oxide is formed from its constituent elements, zinc and oxygen, in their standard states. This value is typically determined experimentally and is found to be around -348.0 kJ/mol.

Why is it important to determine the enthalpy of formation of ZnO?

Determining the enthalpy of formation of ZnO is important because it provides essential thermodynamic data that can be used in various applications, including materials science, metallurgy, and chemical engineering. It helps in understanding the stability and reactivity of ZnO, which is crucial for its use in products like semiconductors, sensors, and catalysts.

What are the common methods used to measure the enthalpy of formation of ZnO?

Common methods for measuring the enthalpy of formation of ZnO include calorimetric techniques such as bomb calorimetry and differential scanning calorimetry (DSC). These methods involve measuring the heat released or absorbed during the reaction of zinc and oxygen to form ZnO. Indirect methods, like using Hess's Law and standard enthalpies of other reactions, can also be employed.

What precautions should be taken during the ZnO formation lab experiment?

During the ZnO formation lab experiment, several precautions should be taken: ensure proper ventilation to avoid inhaling fumes, handle chemicals with care to avoid contamination or reactions, use appropriate personal protective equipment (PPE) such as gloves and safety goggles, and follow all safety protocols for handling high-temperature equipment if calorimetric methods are used.

How do you calculate the enthalpy change from experimental data in the ZnO lab?

To calculate the enthalpy change from experimental data in the ZnO lab, you first measure the temperature change during the reaction. Using the specific heat capacity of the calorimeter and the mass of the reactants, you calculate the heat absorbed or released. This value, along with the stoichiometry of the reaction, allows you to determine the enthalpy change per mole of ZnO formed. The formula used is: ΔH = -q/n, where q is the heat absorbed or released and n is the number of moles of ZnO formed.

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