Answer:
insufficient information in given to solve this question
as per 1st law of thermodynamics, heat transfer and work is related to internal energy of the system which is related to temperature and nothing is said about the temperature change.
hope it helps...pls do upvote
The following reaction was carried out in a bomb calorimeter. The quantity of heat transferred (q)...
Question 16 5 pts The following reaction was carried out in a bomb calorimeter. The quantity of heat transferred (q) for the reaction is -106 kJ. How much work is done by the system? CH4 (8) + 45 (s) – CS2() + 2H2S (8) +106 kJ Cok insufficient information in given to solve the question 106 kJ
2) 1.9 g of an unknown hydrocarbon (44 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter, Cv, = 5.539 kJ/°C and AT =15.874 ºC. Find AE for this hydrocarbon in kJ/mol. (Hint: This is a bomb calorimeter, where the reaction is happening at constant volume: So, what is zero? How is AE related to q (heat)?) Identify: system = Surrounding =
The heat capacity of a bomb calorimeter is found to be 5.25 kJ/degree C. When a 1.94 g sample of glucose (C_6H_12O_6, MM = 180.l6) is burned in the calorimeter, the final temperature recorded was 36.0 degree C. What is the quantity of heat (in kJ) release or absorbed by the reaction if the heat of combustion for glucose is -2.81 times 10^3 kJ/mole. (please include the proper sign in your numerical answer) What is the initial temperature (in degree...
Bomb Calorimetry Worksheet A bomb calorimeter is used to determine the Heat of Formation of an unknown The calorimeter is calibrated using Benzoic Acid initially, Carry out the calculations substance. requested given the following data Material Data Needed: Coo2 28 80 J/mol-K Co.-21.04 J/mol-K С.oo #75 29 JmoLK R 0.08205 L-atm/mol-K AHr(CO2)s-393.51 kJ/mol Calibration Data: Mass of Benzoic Acid: MsA 0.7142 g. MW 122.12 gm/mol, AH-385.1 kJlmol Fuse Wire: AUse 9.62 J/cm Lae 4.4 cm Bomb: Po.-15.0 atm VBoro# 0.500...
A 0.01 mole sample of butane was burnt in a bomb calorimeter The heat from the reaction raised the temperature of 1 kg of water by 6.90°C. How much heat was released by the combustion of this quantity of butane? The specific heat of water is 4.184 J/g-°C. Please select an answer. 28900 J 6900 J 4184 J 29 J
0.500 g of graphite (elemental carbon) is reacted with oxygen in a bomb calorimeter filled with water, which has a total heat capacity of 2820 J/oC. If the reaction gave off 16.4 kJ and the initial temperature of the water and calorimeter was 22.40 oC, what should the final temperature be? I got 34.031 when i tried it using q=mc(tf-ti) and it was wrong. I really need to learn this so as much work as you can help me with,...
A bomb calorimeter is filled with 4.4 atm of an unknown gaseous hydrocarbon fuel and an excess of oxygen gas at a temperature of 21 °C. The bomb calorimeter has a volume of 5 L and a heat capacity of 8.34 kJ/K. After the combustion reaction is complete the final temperature of the calorimeter is found to be 231.6 °C. Answer the following questions based on this information. (a) What amount of heat in kJ was released from the combustion...
Calculate the work (in kJ) done on the system when 2.80 moles of hydrogen gas are produced from the reaction of sodium in excess water at 298 K: 2Na(s) 2H2O()2NaOH(aq) + H2(g) Answer: 2.62 Calculate the work (in kJ) when 1.40 moles of methane react with excess oxygen at 463 K: CH4(g) 202(g) CO2(g) 2H20 (1) Answer: 13.1 1.927 g of an unknown hydrocarbon (129.1 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter,Cv, =...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...