When a 213.0 g sample of aluminum is raised in temperature from 22.0 degrees C to 95 degrees C what amount of heat is produced? 13,994 J 18,211 J 4,217 J 15,549 J
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When a 213.0 g sample of aluminum is raised in temperature from 22.0 degrees C to...
A 3.00-g sample of aluminum pellets (specific heat capacity=0.89 J/°C g) and a 18.50-g sample of iron pellets (specific heat capacity = 0.45 J/°C-g) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 77.4 g water at 22.0 °C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. Final temperature = 20.23 °C An error has been detected in your answer. Check for typos. miscalculations...
Page |62 ADDITIONAL or OPTIONAL QUESTIONS 4. A 150.0 g sample of aluminum, c 0.90 J(gxoC), is heated to 250.0 °C and rapidly dropped into a calorimeter containing 100.0 g of water, c = 4.18 J/(gx°C), at 22.0 °C. What is the final temperature of water in the calorimeter? Assume no heat escaped from the calorimeter
A block of aluminum at a temperature of T1 = 31.5 degrees C has a mass of m1 = 14 kg. It is brought into contact with another block of aluminum with a mass of m2 = 0.5m1, at a temperature of T2 = 15 degrees C. This aluminum has a heat capacity of c = 899 J/kg K. b. What is the temperature in degrees C? c. What was the heat transfer to block 1, in joules?
A 3.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/°C·g) and a 11.00-g sample of iron pellets (specific heat capacity = 0.45 J/°C·g) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 73.8 g water at 22.0 °C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. Please be super specific on how you get to each step!
A 275-g sample of nickel at 100.0°C is placed in 100.0 g of water at 22.0°C. What is the final temperature of the water? Assume no heat transfer with the surroundings. The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C. Hint: The final temp for both the system and surroundings will be the same.
A sample of aluminum absorbs 50.1 J of heat, upon which the temperature of the sample increases from 20.0°C to 35.5°C. If the specific heat of aluminum is 0.900 J/g- °C, what is the mass, in grams, of the sample?
< Question 7 of 19 > The temperature of a sample of aluminum increased by (23.3- \text{°C}\) when (269\text{J}W) of heat was applied What is the mass of the sample? Substance lead silver Specific heat J/g. °C) 0.128 0.235 0.385 0.449 0.903 copper iron aluminum Vm=10) W\text{g} \0
a) calculate the temperature change for a 987 gram sample of water that absorbed 6,990 joules of heat. is this endo- or exorthermic? b) how many grams of water when absorbing 12,000 calories will heat from 31.2 degrees c to 99.5 degrees c? c) 69.8 grams of aluminum is heated with 3,900 joules of energy. what will be the temperature change? what would the temperature be if the initial temperature was 25.0 degrees c? the c for aluminum is =...
7. Calculation of the Amount of Energy Given Off in a Combustion Reaction Section PreLab Questions 1. Aluminum has a specific heat of 0.902 J/g x°C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0 °C to a temperature of 22.0°C? 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of liquid water is 4.18...
The temperature of a sample of iron increased by 24.3 °C when 269 J of heat was applied. What is the mass of the sample? Substance Specific heat J/(g · °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903