to heat 34.4 g g of copper from 122∘C ∘ C to 229 ∘C in Joules
my answer was 1,417.1 ---- I do not think that's right
At 25°C, 230 joules of heat is added to 10.0-g samples of pure gold and copper. Which metal has a higher final temperature?
How many grams of copper can be cooled from 66.8 to 20.3 °C by the heat gained by 100.0 g of water that has an increase in temperature from 24.7 to 33.6 °C? Answer in joules and in calories
The specific heat capacity of solid copper metal is 0.385 J/gK. How many joules of heat are needed to raise the temperature of a 2.12-kg block of copper from 25.0°C to 88.0°C?
How much heat in joules is required to heat a 50 g sample of aluminum from 70 ∘F to 141 ∘F? (The specific heat capacity of aluminum is 0.903 J/(g⋅∘C).) Express your answer using two significant figures.
Part 1: Specific Heat of Copper Metal Your Data Neighbor 1 Neighbor 2 Weight of copper taken, grams 24.724 g __ 24.916 g 25.124 g Weight of water taken, grams 49.591 g_ 50.129 g 24.983 g Temperature of heated copper, 100°C 100°C 100°C Temperature of cool water, °C 22°C 23.2°C 21.5°C Final temperature reached, °C 25.5°C 26.5°C 24.9°C Heat GAINED by water, Joules Heat LOST by copper, Joules Specific heat of copper, Joules/g°C Average value of specific heat of copper...
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g · K and 0.385 J/g · K, respectively.) Final temperature = How much energy is required to raise the temperature of 14.7 grams of gaseous hydrogen from 24.7 °C to 37.7 °C ? Answer: Joules.
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat - 2.46 J/g°C, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
The specific heat of aluminum is 0.900 J/g*C. How many joules of heat are absorbed by 15.0 grams of AI if it is heated from 20.0 C to 60.0 C. Please show how to work out.
How many joules of energy would be required to heat 26.4 g of carbon from 23.6°C to 54.2°C? (Specific heat capacity of carbon = 0.71 J/g.°C.) 1.1 X 103 1.0 X 103 none of these 1.5 X 103 5.7 X 102
The specific heat of copper is 0.385 J/(g °C). If 34.2 g of copper, initially at 25°C, absorbs 7.880 kJ, what will be the final temperature of the copper? 25.4°C 598°C 27.8°C 623°C