A solution is made by mixing252.0 mL of ethanol initially at 11.0 ∘C11.0 ∘C with 252.0 mL252.0 mL of water initially at 21.0 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mLand the density of water is 1.00 g/mL1. The specific heat of ethanol is 2.46 J/g⋅°Cand the specific heat of water is 4.184 J/g·°C.

Q: How many milliliters of water at 21 °C with a density of 1.00 g/mL must be mixed with 220 mL of…

A:

Q: A 3.75 g piece of gold initially at 587.15 K is dropped into 20.6 mL of water at 295.75 K. Calculate…

A:

Q: How much heat, in joules and in calories, must be added to a 75.0–g iron block with a specific heat…

A: Heat is the transfer of energy due to the difference in temperature.

Q: How much heat (in Joules) is gained by 447 grams of water that is warmed from 25.0 J °C to 54.0°C?…

A: The amount of heat absorbed (or released) by fixed amount of a substance to change its temperature…

Q: What is the specific heat of an unknown substance if 1239 j are required to heat 34g of the…

A: Given Heat = 1239 j and mass is 34 gram

Q: What is the final temperature reached by the mixture in the calorimet

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: You take 246 g of a solid (melting point = 38.9 °C, heat of fusion = 425 J/g) and let it melt in 855…

A: Since we are ignoring the specific heat of the solid, we will only consider the heat required during…

Q: 22.214 g of a metal at 99.73°C was added to 14.2 g of water at 19.05°C. The temperature of the…

A: Given: Mass of metal = 22.214 g Initial temperature of metal = 99.73 °C  Mass of water = 14.2 g…

Q: A group of students place 15.41g of a metal into a test tube. They place the test tube into a beaker…

A: Given, mass of the metal = Wmetal = 15.41 g  Mass of the water = Wwater = 10.47 g Initial…