We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Calculate final temp of water when a 3.00 g piece of iron at 85.0°C (Specific heat...
SPECIFIC HEAT OF A METAL Specific heat is an intensive property, which is the amount of heat required to raise the temperature of 1 gram substance by 1°C. Specific heat units areJ/g °C. Solve the following problems using your lecture notes: 1. When 8.50 g of metal, initially at 82 °C, is placed in 45 g water at 20°C, the final temperature of the metal and water is 22 °C. Calculate the specific heat of the metal in J/gºC. (specific...
A 130.0 g piece of copper (specific heat 0.38 J/g・°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature of the copper? (The specific heat of water is 4.18 J/g・°C and the density of water is 1.00 g/mL).
A 50.0 g piece of hot iron is placed in 165 g of water with an initial temperature of 22.8°C. The temperature of the combination rises to 25.7°C. What was the initial temperature of the iron? The specific heat of iron is 0.449 J/gK and the specific heat of water is 4.18 J/gK.
A 248-g sample of copper is dropped into 390 g of water at 22.6oC. The final temperature was measured to be 39.9 oC. Calculate the initial temperature of the copper. Density of water 1.00g/mL. Specific heat of copper = .384 J/g oC
CHM 1210 Final practice Name: Know electrolyte table, 5 solubility rules; 26 polyatomics (name/formula) Write 7 naturally occurring diatomic molecules (name; formula, phase , charge) Write rite out strong acids and weak acids by name; formula, phase ,charge Write out the molecular, complete, and net-ionic equations for the following reactions The mixing of Cobalt(IlI) chloride and silver nitrate The mixing of acetic acid and sodium hydroxide The mixing of hydrochloric acid and cakcium hydroxide The mixing of barium chloride and...
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...
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!
5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both water and iron was measure at 28.5 °C. Calculate the initial temperature of iron? (Specific heat of water and iron from #1)
a 5g piece of lead(specific heat .129 J/gC) is placed in 50ml of water(4.184). water temp incteases from 20 to 22 deg C lead final temp is also 22 deg C what was initial lead temp? please show work, equation used
4. Calculate the heat change in a system (q) when 12.0 g of water is heated from 20.0 °C to 100.0 °C. 5. A 295 g aluminum engine at an initial temperature of 3.00 °C absorbs 85.0 kJ of heat. What is the final temperature of the engine? The specific heat capacity for aluminum is 0.900 J/(g K).