How much heat is absorbed when the temperature of a 4.1 g copper coin increases from 15.3 °C 74.6 °C? The specific heat of copper is 0.385 J/g°C.Question 5Select one:a.142 Jb.93.6 Jc.5.57 Jd.632 J
Question
How much heat is absorbed when the temperature of a 4.1 g copper coin increases from 15.3 °C 74.6 °C? The specific heat of copper is 0.385 J/g°C.Question 5Select one:a.142 Jb.93.6 Jc.5.57 Jd.632 J
Solution
To solve this problem, we need to use the formula for heat transfer which is:
q = mcΔT
where:
- q is the heat absorbed,
- m is the mass,
- c is the specific heat, and
- ΔT is the change in temperature.
Given:
- m = 4.1 g,
- c = 0.385 J/g°C, and
- ΔT = 74.6°C - 15.3°C = 59.3°C.
Substituting these values into the formula gives:
q = (4.1 g)(0.385 J/g°C)(59.3°C) = 93.6 J.
So, the heat absorbed when the temperature of a 4.1 g copper coin increases from 15.3 °C to 74.6 °C is 93.6 J. Therefore, the correct answer is b. 93.6 J.
Similar Questions
The molar mass of copper is 63.546 g/mol. The specific heat of copper is 0.385 How much heat is released when 0.762 mol of copper cools from 81.6°C to 52.2°C? a 973 J b 548 J c 8.63 J d 93.7 J
The specific heat of copper is 0.385 J/(g ∙ °C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper?Group of answer choices125 °C266 °C300 °C381 °C
How much heat is absorbed when 15.0 g of liquid water is heated until the temperature increases by 6.0°C? The specific heat of liquid water is 4.18 J/g°C. a 376 J b 212 J c 194 J d 22 J
The specific heat of copper is 387 J/kg°C. The temperature of a 0.45-kg sample of copper decreases from 86.0 °C to 20.0 °C. How much heat flows out of the copper sample during this temperature drop? 8,700 J 9,600 J 11,000 J 14,000 J
Copper is a type of metal. A block of copper has a mass of 2.0 kg. The block of copper absorbs 12000 J of thermal energy. The specific heat capacity of copper is 385 J/(kg°C). What is the temperature rise of the copper?
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.