Water has a specific heat of 4.184 J/g deg while glass (Pyrex) has a specific heat of 0.780 J/g degree. If 10.0 J of heat is added to 1.00 g of each of these, which will experience the larger increase in temperature?
Correct answer: A. Glass
- A. Glass
- B. Water
- C. They both will experience the same change in temperature since only the amount of substance relates to the increase in temperature
- D. None
Explanation
The correct answer is Glass. The specific heat capacity of a substance tells us how much energy is required to change the temperature of a unit mass of the substance by one degree Celsius. Glass has a specific heat of 0.780 J/g°C, which is lower than water's specific heat of 4.184 J/g°C. This means that for the same amount of heat added, glass will experience a larger increase in temperature compared to water because it requires less energy to change its temperature. The other options are incorrect because they do not take into account the influence of specific heat capacity on the temperature change.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
Practise Thermochemistry and Energetics of Chemical Reactions
728 free Thermochemistry and Energetics of Chemical Reactions MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Thermochemistry and Energetics of Chemical Reactions questions
If 1 J of heat is added to a 2.00 g sample of aluminum metal, and the temperature of the metal increases by 1°C, what is the specific heat of aluminum?
If a system loses 250 kJ of heat at the same time that it is doing 500 kJ of work, what is the change in the internal energy of the system?
A 100g sample of water at 25 °C and 1 atm. of pressure. Then, 100g of water that has recently heated to 100 °C from 0 °C and then cooled to 25 °C at 1 atm. of pressure.
The heat of combustion for 1 mole of carbon to carbon dioxide is -410 kJ. How many kJ of heat would be liberated from the complete combustion of 60.0 g of carbon?
Given the following data at 1 atm of pressure and 25.0 °C...ΔH°formation = +64.4 kJ/mole for Cu²⁺.ΔH°formation = -152.4 kJ/mole for Zn²⁺.ΔH°formation = 0 for both Zn and Cu²⁺ because these are in the most stable state.Calculate the standard heat of reaction for........Zn(s) + Cu2+ (aq) →Zn2+(aq) + Cu(s)
Which statement describes characteristics of an endothermic reaction?