heat lost by hot silver = heat gained by water
m1*s1*DT1 = m2*s2*DT2
m1 = mass of hot silver = 362 g
S1 = specific hot silver = 0.031 j/g.c
DT1 = 58
m2 = mass of water = 98.56 g
S = specific heat of water = 4.184 j/g.c
DT2 = x-23.4
362*0.031*58 = 98.56*4.184*(x-23.4)
x = 24.98
x = final temperature of water = 24.98 c
The temperature of a piece of silver (specific heat Sag = 0.031j/g.°C) with a mass of...
PLEASEEE HELPPP ASAPP 6- (15 pts) The temperature of a piece of silver (specific heat Se=0.031/8."C) with a mass of 362 g decreased by 58 °C when it was added to a 98.56 g sample of water (specific heat of water 5, 4.184 1/8 'C) in a constant pressure calorimeter of negligible heat capacity. What is the final temperature of water if its initial temperature was 23.4 "C?
6. A piece of 155.0 g aluminium metal at 120°C was placed in a constant pressure calorimeter of negligible heat capacity containing 300.0 g of water at 20°C. Calculate the final temperature of the system (the aluminium metal and the water) in °C: given the specific heat of aluminium metal = 0.90 J/g °C, and that of water 4.184 J/g °C
Calculating specific heat capacity A constant-pressure calorimeter is often used to find the specific heat capacity of a substance if it is not known. A known mass of the substance can be heated and added to water of known mass and initial temperature. Since the specific heat capacity of water is known ( C s,water =4.184J/(g⋅ ∘ C)) , the amount of heat transferred to the water can be calculated by measuring the final temperature of the mixture at thermal...
One piece of silver jewelry, at T1= 985.8°C, has three times the mass of another piece (3m1= m2) at TI= 120.0 °C. Both are placed in a calorimeter of negligible heat capacity. What is the final temperature inside the calorimeter (C = 0.233 J/g°C)?
18. When a piece of copper at a temperature of 256.0 °C is added to 255 grams of water at a temperature of 20.0 °C, the final temperature of the resulting mixture is 24.0 °C. If the specific heat capacity of copper is 0.385 J/g°C, calculate the mass of the piece of copper used in the experiment? The specific heat capacity of water is 4.184 J/ g• °C. (5 points)
What is als? Assume that no heat is lost to the surroundings (Hint: The heat gained by the gold must be equal to the heat lost by the iron. The specific heats of the metals are given in Table 6.2.) To a sample of water at 23.4°C in a constant- 6.36 pressure calorimeter of negligible heat capacity is added a 12.1-g piece of aluminum whose tempera- ture is 81.7°C. If the final temperature of water is 24.9°C, calculate the mass...
A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity = 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 5.445 g is quickly added. The salt has a molar mass of 250.465 g/mol. The final temperature of the solution is 33.49 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the solution is equal...
A 20.0g piece of metal with a specific heat L Thermochemistry 1. Calculate the total change in internal energy. AE of a system when 400 J heat is oplies to expanding O2(g) and the gas does 350 J of work on its surroundings. 2. Calculate the kinetic energy in .colories, and 6.00x10 m/s. of a portice (moss 9.11x109) 3. Calculate AH in kJ for reaction. CO CO given the following thermochemical data: 2CO(g) + 020) ► 2C0z9) AHP:. 566.1 kJ...
Question 4 of 8 > Substance lead Specific heat capacity (J/g °C) 0.128 0.235 0.385 silver copper iron 0.449 aluminum 0.903 4.184 water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 18.3 °C when 81.3 J of heat is added to the substance. What is the most likely identity of the substance? O aluminum silver O water O copper
A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity = 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 5.451 g is quickly added. The salt has a molar mass of 124.742 g/mol. The final temperature of the solution is 73.937 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the solution is equal...