Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔHorxn = -802.3 kJ You may want to reference (Page 269) Section 6.6 while completing this problem.What minimum mass of CH4 is required to heat 85.0 g of water by 23.0 ∘C? (Assume 100% heating efficiency.) (For water,Cs= 4.18 J/g∘C).
CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔHorxn = -802.3 kJ
m = 85g
cs = 4.18J/g-0C
T = 230c
q = mcT
= 85*4.18*23
= 8171.9J
= 8.1719KJ
The combustion energy of CH4 = 802.3Kj/mole
8.1719KJ/802.3Kj/mole = 0.010186 moles of CH4
mass of CH4 = no of moles * gram molar mass
= 0.010186*16 = 0.163g of CH4
Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔHorxn =...
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Review Coristas Petole Table Natural gas burns in air to form carbon dioxide and water releasinghe CH,(s) +0,6) - CO.(a)+H06) AH-812.3. Part A What minimum mass of CH is required to heat 800 g of water by 26.0°C? (Assume 10015 heating efficiency) (For water. = 4.18 J/C) 1745 4,00 x 10' 0.1748 Suomi Rest
What mass of natural gas (CH4) must you burn to emit 258 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ
For the reaction CH4 + 2O2 → CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 97.0 g of methane?
What mass of natural gas (CH4) must you burn to emit 259 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Express the mass in grams to three significant figures.
Methane (CH4) burns in air to form carbon dioxide and water as shown below. CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) If a sample of methane occupies 426. mL at 2.31 atm, what volume (in mL) of oxygen gas at the same temperature and pressure is required to complete the reaction?
Balanced equation: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Part B: What mass of carbon dioxide is produced from the complete combustion of 2.70×10−3 g of methane? Part C: What mass of water is produced from the complete combustion of 2.70×10−3 g of methane? PartD: What mass of oxygen is needed for the complete combustion of 2.70×10−3 g of methane?
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.10 g of methane is combusted at constant pressure.
Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction: 2H,C - CH3(g) + 702(g) +4CO2(g) + 6H2O(g) Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol Use average bond energies to calculate AH.. for this reaction. Η ΑΣΦ « ο ο _ ? ΔΗ,