What change in temperature results when 2500 Joules of heat is applied to a 7.00 gram...
How much heat (in joules) is used to heat a 53.30 gram sample of iron from 14.7 degrees Celcius to 100.00 degrees Celcius if the specific heat of Fe is 0.450 J/g°C? J
solve The heat energy associated with a change in temperature that does not involve a change in phase is given by -msAT where q is heat in joules, mis mass in grams, s is specific heat in joules per gram-degree Celsius, J/(g·°C). and AT is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by where q is heat in joules, m is mass in grams, and ? H...
a) calculate the temperature change for a 987 gram sample of water that absorbed 6,990 joules of heat. is this endo- or exorthermic? b) how many grams of water when absorbing 12,000 calories will heat from 31.2 degrees c to 99.5 degrees c? c) 69.8 grams of aluminum is heated with 3,900 joules of energy. what will be the temperature change? what would the temperature be if the initial temperature was 25.0 degrees c? the c for aluminum is =...
the Specific Heat Capicity of Tungsten is given here. 3. Calculate the temperature change when 32 grams of tungsten has 21 Joules of heat added to it. temperature be- in between the initial temperatures of the t and will be the same for the metal and the water.) Table 1. Specific heat capacities of various metals and other substances Specific Heat Capacity, C (J/g.°C) 0.129 0.129 0.132 0.133 Specific Heat Capacity, C (3/goC) 0.421 0.444 0.449 0.450 0.460 0.522 0.757...
1. In the laboratory a student finds that it takes 81.6 Joules to increase the temperature of 14.1 grams of solid iodine from 25.0 to 39.4 degrees Celsius. The specific heat of iodine calculated from her data is J/g°C. 2. In the laboratory a student finds that it takes 116 Joules to increase the temperature of 11.8 grams of solid sulfur from 24.0 to 38.1 degrees Celsius. The specific heat of sulfur calculated from her data is J/g°C. 5.1
1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C. 2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the...
1. An unknown sample is being evaluated in lab. What is the specific heat of the compound if it requires 105.06 J to raise the temperature of 51.68 grams of the unknown from 15.25 °C to 22.9 °C. 2. A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celsius is added to 50.00 grams of water initially at 5.94 degrees Celsius. The final temperature of the system is 20.15 degrees Celsius. Calculate the specific heat of the...
Energy/Specific Heat (q=mcAT) 1. Determine the energy, in Joules, needed to increase the temperature of 20.00 g of water from 300.0 K to 365.0 K. (Remember that one degree of Celsius contains the same amount of energy as one Kelvin.) 2. Determine the energy, in Joules, released as 1.00 kilogram of water cools from 72.0°C to 30.0°C. 3. 25.0 g of mercury are heated from 25.0° C to 155.0°C and absorbs 455 joules of heat in the process. Calculate the...
answers should have correct significant figures. All four questions use the equation q = MCAT 1. How much energy is absorbed by a 70.0g sample of water being heated from 18 degrees Celsius to 100 degrees Celsius, given the heat capacity of water as 4.184J per gram degrees Celsius. 2. If a 20.0g sample of gold absorbed 250.0 Joules of energy, what was the change in temperature given a heat capacity for gold as 0.129J per g degrees Celsius? 3....
A 61.93 gram sample of iron (with a specific heat of 0.450 J/g °C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 40.6 g of water (specific heat of 4.184 J/ g °C) initally at 20.63 °C. If the final temperature of the system is 23.59, what was the heat absorbed (q) of the calorimeter? (total heat absorbed by the water and calorimeter = heat released by the iron)