1. A 2.80 g lead weight, initially at 11.0 ∘C, is submerged in 8.19 g of water at 53.0 ∘C in an insulated container.
What is the final temperature of both the weight and the water at thermal equilibrium?
2. It takes 45.0 J to raise the temperature of an 9.60 g piece of unknown metal from 13.0∘C to 24.6 ∘C. What is the specific heat for the metal?
3. The molar heat capacity of silver is 25.35 J/mol. ∘C. How much energy would it take to raise the temperature of 9.60 g of silver by 17.1 ∘C?
4. What is the specific heat of silver?
In the ist part , specific heat capacity of metal Pb is not given . Without this we cannot calculate final temperature. Thus i have supposed specific heat of Pb is x. I have solved rest of the part . You have to just plug in the value of x and you will be able to calculate final equilibrium temperature.
1. A 2.80 g lead weight, initially at 11.0 ∘C, is submerged in 8.19 g of...
A 2.94 g lead weight, initially at 11.1 ∘C, is submerged in 7.72 g of water at 51.8 ∘C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium?
A 2.40 g lead weight, initially at 10.5 ∘C, is submerged in 8.08 g of water at 52.1 ∘C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium?
A 6.66 g lead weight, initially at 9.3 oC, is submerged in 10.00 g of water at 52.3 oC in an insulated container. What is the final temperature of both substances at thermal equilibrium? Specific heat capacity of lead = 0.128 J/gC; water = 4.18 J/gC O A. 52.3 oC OB. 51.4 OC OC. 53.6 oC OD. 49.4 oC OE. 50.3 oC OF. 47.6 OC O G. 48.4 oC OH. None of the above
A silver block, initially at 56.4 ∘C, is submerged into 100.0 g of water at 24.6 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.4 ∘C. What is the mass of the silver block?
A 2.58 g lead weight, initially at 10.4 ∘C, is submerged in 7.85 g of water at 52.3 ∘C in an insulated container. e What is the final temperature of both substances at thermal equilibrium?
A2.13 g lead weight, initially at 11.1°C, is submerged in 7.45 g of water at 52.5 °C in an insulated container Part A You may want to reference (Pages 373 - 379) Section 9.4 while completing this problem. What is the final temperature of both the weight and the water at thermal equilibrium? Express the temperature in Celsius to three significant figures. AEC RO? Submit Request Answer
a.) It takes 52.0J to raise the temperature of an 9.60 g piece of unknown metal from 13.0 degrees Celsius to 24.2 degrees Celsius. What is the specific heat for the metal? The next two questions pertain to silver. They have nothing to do with unknown metal described in Part A. b.) The molar heat capacity of silver is 25.35 J/mol * degrees Celsius. How much energy would it take to raise the temperature of 9.60g of silver by 18.6...
1. A 31.6 g wafer of pure gold initially at 69.4 ∘C is submerged into 63.8 g of water at 27.7 ∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium? 2.Two substances, A and B, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of substance A is 6.04 gand its initial temperature is 21.0 ∘C . The mass of substance B is 25.5 gand its initial temperature is...
A silver block, initially at 58.6 ∘C, is submerged into 100.0 g of water at 25.1 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.3 ∘C. What is the mass of the silver block? I got 122.53g is it wrong?
A) A silver block, initially at 55.4 ∘C, is submerged into 100.0 g of water at 25.3 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.8 ∘C. What is the mass of the silver block? B) Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.50×102kJ of heat? The balanced chemical equation is as follows: C(s)+O2(g)→CO2(g),ΔH∘rxn=−393.5kJ