The calorimeter constant for a certain constant-volume calorimeter was determined to be 69.3J*K-1. By how much will the temperature rise when 0.01350g of phenol, C6H5OH (s), is burned in the calorimeter? This calorimeter uses 2000g of water (Mm(H2O) = 18.02g*mol-1).
DeltafH(CO2, g) = -393.51 kJ *mol-1 ; delta fH(H2O, l) = -285.83 kJ*mol-1 ; delta fH (C6H5OH, s) = -165 kJ*mol-1 ; Cp.m (H2O) = 75.48 J*mol-1.
The calorimeter constant for a certain constant-volume calorimeter was determined to be 69.3J*K-1. By how much...
A sample of solid pyrene (C16H10) that weighs 0.5063 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.130 °C. The heat capacity of the calorimeter and its contents is known to be 9.233×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
A sample of solid 1,9-nonanediol (C9H20O2) that weighs 0.5724 g is burned in an excess of oxygen to CO2(g) and H2O(l) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.210 °C. The heat capacity of the calorimeter and its contents is known to be 9.268×10^3 J K^-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Please specify states such as (aq) or (s). ____+____--->____+____ Based on...
A sample of solid bianthracene (C28H18) that weighs 0.5275 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.170 °C. The heat capacity of the calorimeter and its contents is known to be 9.520×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Based on this experiment: (b) Assuming that H° is approximately equal...
A sample of solid 1,2-benzenediol (C6H6O2) that weighs 0.8129 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.270 °C. The heat capacity of the calorimeter and its contents is known to be 9.301×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction.Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s)....
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4395 g sample of biphenyl (C12H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.064×103 g of water. During the combustion the temperature increases from 26.33 to 29.52 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was...
A sample of solid diphenyl phthalate (C20H14O4) that weighs 0.6847 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.110 °C. The heat capacity of the calorimeter and its contents is known to be 9.580×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq)...
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.5691 g sample of 1,2-benzenediol (C6H6O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.322×103 g of water. During the combustion the temperature increases from 22.82 to 25.02 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was...
1. 2. A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.425-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from...
1. 2. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods In an experiment, a 0.3568 g sample of bianthracene (C28H18) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.030x10 g of water. During the combustion the temperature increases from 25.45 to 28.29 °C. The heat capacity of water is 4.184 J gC The heat capacity of the...
Thermometer Ignition wires heat sample Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Water In an experiment, a 0.3916 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.266x10 g of water. During the combustion the temperature increases from 23.47 to 26.10 °C. The heat capacity of water is 4.184 J gloc-1....