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A chunk of mercury at 80.8°C was added to 200.0 g of water at 15.5°C. The...
PLEASE EXPLAIN ALL STEPS! A chunk of aluminum at 200.0 °C was added to 43.0 g water at 20.0 °C. The final temperature is 35 °C? What is the mass of aluminum that was added?
146 g of water at 76.5 degree C are mixed with 75.4 g of water at 21.5 degree C. If no heat is lost to the surroundings, what is the final temperature of the water? The specific heat of water is 4.184 J/g degree C.
15. A coffee cup calorimeter contains 400.0 g of water and 25.0 g of ice at 0.0 °C. When a 35.00 g scoop of calcium chloride (also at 0.0 °C) is added to the ice water, the calcium chloride dis- solves as shown. The heat produced by this reaction is enough to melt all of the ice and warm up the resulting calcium chloride solution. What is the final temperature of this solution? Assume there is no heat lost to...
2. Solid mercury at -89 °C is added to liquid water at 0°C. When the system reaches thermal equilibrium all the water is ice and half of the original mercury is liquid. Assume that no heat is lost to the surroundings and find the ratio of the mass of mercury to the mass of water (mHg/m1,0). Melting Point Heat of Fusion Heat Capacity (solid) (°C) (J/kg) (J/kg.Cº 0.10 x 105 140 3.00 x 105 2000 Mercury Water -39 0
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.
Question 10 2 pts If 15.5 J of heat are removed from 14.6 g of mercury (specific heat 0.142 J/g °C) at 25.0 °C, what is the final temperature of the mercury sample in °C? (Give only the numerical value in the box)
An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a glass containing 4.20×102 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, ?s , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, Δ?∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings.
An ice cube with a mass of 53.0 g at 0.0 °C is added to a glass containing 368 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g·°C and the standard enthalpy of fusion, ΔH°fus, of water is 6.01 × 103 J/mol. Assume that no energy is transferred to or from the surroundings.
11. A calorimeter contains 12.0 g of water at 57.0 °C. If a 4.00 g chunk of gold at 18.2°C is placed in the water, what is the final temperature of the water in the calorimeter? (The specific heat of gold is 0.128 J/g °C.)!
Path: P Words:0 QUESTION 27 A 42.9 g sample of Fe (specific heat 0.449 J/gºC) at an initial temperature of 125.0°C is added to 185.0 g sample of water. The final temperature reached for both is 42.1°C. Assuming no heat is lost to the surroundings and given that the specific heat of water is 4.18J/g°C, what is the initial temperature of the water, in °C? Simply type the number, not the unit. QUESTION 28