A .500g sample of KCl is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved in the dissolution of .500g KCl, assuming the heat capacity of the solution is 4.184J/g degrees celsius?
A .500g sample of KCl is added to 50g of water initially at 25 degrees celsius...
A .500g sample of KCL is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved per mol of KCL?
A 0.400 g sample of KCl(s) is added to 50.0 g of water in a calorimeter. If the temperature decreases by 0.95˚C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g˚C?
A 0.400 g sample of KCl(s) is added to 50.0 g of water in a calorimeter. If the temperature decreases by 0.95˚C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g˚C?
A 50g sample of iron is heated to 75.2°C and placed into a calorimeter holding 70g of water at a temperature of 25°C. Assuming no heat loss to the calorimeter, what will be the final temperature reached in the calorimeter? Specific heat capacity of iron = .444J/g•C° Specific heat capacity of water = 4.184J/g•C°
When a 3.00-g sample of KCl was added to 3.00 × 102 g of water in a coffee cup calorimeter, the temperature decreased by 1.05 °C. How much heat is involved in the dissolution of the KCl? please show work thank you
A 70g sample of water at 25 Celsius is mixed with 50g of a certain metal at 100 Celsius. After thermal equilibrium was established, the temperature of the mixture is 29.6 Celsius. What is the specific heat capacity of the metal? show work please
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 12.16 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C). (HINTS: Recall that the q of a system is equal to the -q of the surroundings. So you can set up two equations here: one for the loss...
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 14.37 degrees Celsius. The final temperature of the metal and water is 20.15 degrees Celsius Calculate the specific heat of the metal (The specific heat of water is 4.184J'g'C). (HINTS Recall that the qof a system is equal to the of the surroundings So you can set up two equations here one for the loss of heat from...
an ice cube at 0.00 degrees celsius with a mass of 4.52 g is placed into 55g of water, initially at 23 degrees celsius. If no heat is lost to the surroundings, what is the final temperature of the entire water sample after all the ice is melted? (Specific heat of water is 4.184J/g*degrees celsius)
A 0.500g sample of C7H5N2O6 is burned in a calorimeter containing 600 g of water at 20 .0 degrees celicus . if the hear capicity of the bomb calorimeter is 420J/c and the heat of combustion at constabt volume of the sample is -3374 kj/mol ,calculate temperature of reaction in Celisus . specfic heat capacity of water is 4.184J/g degress celsius