Magnesium metal is added to a coffee cup calorimeter containing 105.0 mL of 2.50 M hydrochloric acid. The temperature increased by 8.2°C. What lesson metal is placed in the calorimeter meter? Look at pic. The heat capacity and density a solution in the calorimeter is the same as those of water: 4.184 J/(g x degrees Celsius ) and 1.00 g/mL. Illinois it change in massive solution caused by adding magnesium and by escape of the hydrogen

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Calculate the heat capacity (in J/°C) of 20.0 ml of room temp. water given that the specific heat capacity of water is 4.184 J/°C g. The density of water at room temp. is 0.9971 g/mL.

chemistry [References] TUTOR Coffee Cup Calorimetry: Specific Heat I In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 66.74 grams of nickel to 98.38 °C and then drops it into a cup containing 78.65 grams of water at 20.69 °C. She measures the final temperature to be 26.85 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.80 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of nickel. Metal sample Specific Heat (Ni) = J/g °C. Show Approach Show Tutor Steps Submit Submit Answer Try Another Version 10 item attempts remaining Previous Ne

If a 50.0g sample of Cu is heated to 180.00C and is placed in 100.0 ml of water in a calorimeter at 25.00C, what will the final temperature be for the system? Assume that all of the heat goes from the copper to the water. (None is lost to the surroundings or calorimeter.) dH20 =1.00g/ml C Cu = 0.385J/goC CH2O = 4.184 J/goC

In a coffee-cup calorimeter, 130.0 mL of 1.1 M  NaOH and 130.0 mL of 1.1 M  HCl are mixed. Both solutions were originally at 20.7°C. After the reaction, the final temperature is 28.1°C. Assuming that all the solutions have a density of 1.0  g/cm3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction, 3 the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ - kJ/mol

A 67.75 gram sample of iron (with a heat capacity of 0.450 J/g °C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 42.29 g of water (specific heat of 4.184 J/ g °C) initially at 20.63 °C. If the final temperature of the system is 23.59, how much heat was absorbed by the calorimeter? Record your answer as a whole number (assume the sign is positive). Submit Question div Mach k Air 20 F1 F2 F3 F4 F7 %24 %23

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2) When 100 g of unknown metal at 100 °C added to a calorimeter containing 50.00 g of water the temperature rises from 24.00°C to 36.54°C. Calculate the specific heat of the unknown metal in J/°C. The specific heat of water is 4.184 J/g °C.