8.502 1S . The temperature of a sample of water increases by 69.5 °C when 24...
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? = 8.50215 2. The temperature of a sample of water increases by 69.5 °C when 24 500 J are applied. The specific heat of...
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...
What is the final temperature when a 10.0 g sample of water is heated with an input of 20.0 kJ starting at 10.0°C? You might need the following information for water: specific heat H2O(s): 2.09 J/g°C specific heat H2O(l): 4.18 J/g°C specific heat H2O(g): 1.84 J/g°C heat of fusion: 6.09 kJ/mole heat of vaporization: 40.7 kJ/mole Answer choices are: 488°C 273°C 89.0°C 100.°C It said 488 was wrong.
The temperature of a sample of silver increased by 22.5 °C when 263 J of heat was applied. What is the mass of the sample? Substance lead silver copper iron aluminum Specific heat J/g °C) 0.128 0.235 0.385 0.449 0.903 m 8
LAB 10 PRE LAB WORKSHEET Specific Heat Capacity (C) The energy transferred as heat that is required to raise the temperature of 1 gram of a substance by 1 kelvin. q= - m x Cp X AT q=heat lost or gained, m= mass of solution (grams) Cp = the Specific Heat Capacity of a compound (J/g x °C)) AT = Tfinal-Tinitial AHsolution = 9 moles of salt 1. If 1.25 g of ammonium nitrate (NH4NO3) is dissolved in 25.0 mL...
16.41 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.7°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g・°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
#6 When 108 g of water at a temperature of 21.1 °C is mixed with 65.7 g of water at an unknown temperature, the final temperature of the resulting mixture is 47.6 °C. What was the initial temperature of the second sample of water? (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.) Initial temperature = °C
16) When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is _______J. (The specific heat of water is 4.18 J/g-°C.)
A calorimeter contains 26.0 mL of water at 13.5 ∘C . When 2.50 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
A calorimeter contains 25.0 mL of water at 13.0 ∘C . When 2.40 g of X (a substance with a molar mass of 64.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...