due soon!! I TUR Check my work Enter your answer in the provided box. High-purity benzoic...
Enter your answer in the provided bos. High-purity benzoic acid (C.H.COOH; AH for combustion --3227 kJ/mol) is used as a standard for calibrating bomb calorimeters. A 1.221-g sample burns in a calorimeter (heat capacity -1365 J°C) that contains exactly 1.390 kg of water. What temperature change is observed? DET PC < Pfly of 16 !! Next hp
High-purity benzoic acid (C6H5COOH; ΔHrxn for combustion = −3227 kJ/mol) is used as a standard for calibrating bomb calorimeters. A 1.221-g sample burns in a calorimeter (heat capacity = 1365 J/°C) that contains exactly 1.350 kg of water. What temperature change is observed? C?
Enter your answer in the provided box. The enthalpy of combustion of benzoic acid (CH COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 3.0653 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84°C to 24.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.) kJ/°C
with correct ammount of sigfigs please
1 attempts left Check my work Enter your answer in the provided box. The enthalpy of combustion of benzoic acid (CH,COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 3.0081 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84°C to 25.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water...
The enthalpy of combustion of benzoic acid ( CH2COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 3.2157 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84°C to 24.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.) kJ/°C
(1) (3 points ) A 1.21 g sample of benzoic acid, C7H602, is combusted in a bomb calorimeter in an oxygen rich environment. The calorimeter has a heat capacity of 1365 J/°C, and additionally contains 1.30 kg of water surrounding the bomb. The heat of combustion for benzoic acid is AH° = -3227 kJ per mole of benzoic acid. The initial temperature of the calorimeter and water is 22.5 °C. a. (1 point) What is the balanced chemical reaction that...
The enthalpy of combustion of benzoic acid (CH-COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters, its value has been accurately determined to be -3226.7 kJ mol! (a) When 0.9862 g of benzoic acid was oxidized, the temperature rose from 21.84°C to 25.67°C. What is the heat capacity of the calorimeter? (b) In a separate experiment, 0.4654 g of glucose (C6H120) was oxidized in the same calorimeter, and the temperature rose from 21.22°C to 22.28°C. Calculate the...
A 1.9862-g sample of benzoic acid burns in an excess of oxygen, in a bomb calorimeter. The temperature of the calorimeter rises from 24.94 C to 28.77 C. The calorimeter contains 2000.0 g of H2O, and the heat capacity of the calorimeter (excluding the water, but including the bomb, thermometer, and all mechanical parts) has the value C(cal) = 5.35 kJ/C. Use the given information to find the molar heat of combustion of benzoic acid (M(benzoic acid) = 122.1 g/mol).
Enter your answer in the provided box. A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 4.46°C. If the heat capacity of the bomb plus water was 9.20 kJ /°C, calculate the molar heat of combustion of methanol. kJ/mol
Enter your answer in the provided box. A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.14°C. If the heat capacity of the bomb plus water was 9.41 kJ / °C, calculate the molar heat of combustion of methanol. kJ/mol