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CREDIT Show all work for partial credit. 1) How much heat energy is released when 1000....
Burning 1.00 mol of methane releases 803 kJ of energy. How much energy is released by burning 27.3 mol of methane? CH, (g) +202(g) + CO2(g) + 2H2O(g) + 803 kJ Express your answer with the appropriate units. E- Value Units Submit Request Answer
4) What mass of natural gas (CH4) must burn so that the heat released by the reaction CH4(g)2 O2(g) CO2(g)+2 H20(g) is 267 kJ. The molar mass of CH4 is 16.0 g mol. The standard enthalpies of formation of some of the substances in the reaction are: AH (CH (g))-74.81 kJ mol AH (CO2(g)-393.509 kJ mol AHP(H20(g)-241.818 kJ mol a) 0.223 g b) 3.57 g c) 0.280 g d 0.623 g e) 1195 g f) 467 g
Burning 1.00 mol of methane releases 803 kJ of energy. How much energy is released by burning 27.7 mol of methane? CH4(g)+2O2(g)→CO2(g)+2H2O(g)+803kJ Express your answer with the appropriate units.
given the following thermochemical equation detailing the combustion of methane (CH4) determine the amount of energy released when 1.563 mol of methane undergoes combustion Given the following thermochemical equation 14. detailing the combustion of methane (CH4) CH g)+ 202(g) CO2(g) + 2H20(g) 1.563 determine the amount of energy released when 1.563 mol of methane undergoes combustion. AH=-802kJ/mol CH a. 1.95 x d. 1250 kJ b. 3,12x 10 kJ e. 2.01 x 10' kJ c. 453 kJ
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, =...
AH CO t H20 AR CHA -398-5 t CHAG) 203 6 + 74-5 2AI Question 3 The combustion of methane is given by: CH (g)+ 2 O2 (g)-CO2 (g) + 2 H20 (g) The flue gases leave the reactor at 800°C. (a) Calculate the heat of reaction at 800°C? (5 point) 5c0 -8K Substance AHP298.15 (kJ/mol) C,IR=A A CH4 -74.5 1.13 3.64 CO2 -393.5 5.46 -241.8 3.47 OH (b) Calculate the amount of heat needed (kJ) to raise the temperature...
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) AH = -1652 kJ (a) How much heat is released when 3.54 mol iron are reacted with excess O2? Ok] (b) How much heat is released when 1.48 mol Fe2O3 is produced? CJ) (c) How much heat is released when 2.50 g iron are reacted with excess O2? DJ (d) How much heat is released when 12.6 g Fe and 1.02 g O2 are reacted? CkJ
Problem 2 CH 25 C Products 150 C Air 100 25 C Cooling water Methane (CH4) is oxidized with air to produce formaldehyde (HCHO) in a continuous reactor via the following reaction: A competing reaction is the combustion of methane to form CO2: In this specific problem, CH4 and O2 enter the reactor at a mole ratio of 1:1. In the reactor, 40% of CH4 is consumed. Of this 40%, 75% reacted via reaction (1) and the other 25% reacted...
- O CO Thermochemical equations Thermochemical s are chemical S tions that day show the relationship between mass of products and reactants and enthalpy changes. For example C4 () + 2O (G) ng) + 2H20 (0) AH = -890 A kJ moles of O2 = -890 A kJ 2 moles of 2H20 = -890.4 kJ - 890.4 kJ - 890.4 kJ mol _moles of CH = - 890.4 kJ I moles of CO2 = - 890.4 kJ - 890.4 kJ...
3. (20) Fire Heater Specification After the reactor feed leaves the heat exchanger, it enters a fire heater. In this unit the stream is further heated from 215°C to 350°C, which requires 4649 kJ/h of heat to be added. To accomplish this, the heat from the combustion of methane gas is used: CH4(2) +2 02(g) → CO2() + 2 H20(2) $ = 10.0 molh The design of this fire heater indicates that the temperature of the flue gas will not...