A hot lump of 38.8 g of aluminum at an initial temperature of 69.2 °C is placed in 50.0 mL H,O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g-°C)? Assume no heat is lost to surroundings. Tinal = °C

A hot lump of 38.8 g of aluminum at an initial temperature of 69.2 °C is placed in 50.0 mL H,O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g-°C)? Assume no heat is lost to surroundings. Tinal = °C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

105 mL of H2 O is initially at room temperature (22.0° C). A chilled steel rod at 2.0° C is placed in the water. If the final temperature of the system is 21.3 °C, what is the mass of the steel bar? Specific heat of water = 4.18 J/g.°C Specific heat of steel = 0.452 J/g.°C
A piece of titanium metal with a mass of 21.6 g is heated in boiling water to 99.5 °C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.8 °C. When thermal equilibrium is reached, the final temperature is 24.5 °C. Calculate the specific heat capacity of titanium. (The specific heat capacity of liquid water is 4.184 J/g. K.) Specific heat capacity= J/g. K
What is the amount of heat (value of q) when 22.8 g of aluminum is heated from 20.0℃ to 425℃? The specific heat capacity of aluminum is Cs,Al = 0.900 J/g℃.
A 46.9-g iron rod, initially at 18.6 oC is submerged into 50.4 g of water at an unknown initial temperature. The final temperature of the mixture upon reaching thermal equilibrium is 69.6 oC. What is the initial temperature of the water (in oC)? The specific heat capacity of iron is 0.449 J/g.oC The specific heat capacity of water is 4.184 J/g.oC
4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)
Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water initially at 22.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C ?f= ∘C
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 100.0 g of water at 25.0 °C, the final temperature is 37.0 °C. What is the specific heat of the alloy? The specific heat of H20(1) is 4.184 J'g-1.°c-1. q = mc AT O A. 0.423 J-g-1.°c-1 O B. 9.88 J-g-1.°C-1 O C. 48.8 J'g-1.°C-1 O D. 1.77 Jg-1.°c-1