How much heat is released when 6.00 g of methane is combusted using the reaction below?
CH4 + 2O2 → CO2 + 2H2O ΔHrxn = -890. kJ
I came up with 334 kJ but not sure if it is correct.
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How much heat is released when 6.00 g of methane is combusted using the reaction below?...
How much heat is released when 6.00 g of methane is combusted using the reaction below? CH4 + 2O2 → CO2 + 2H2O ΔHrxn = -890. kJ I got 334kJ, but it is multiple choice and my answer can be positive or negative...I am just not sure which one.
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.
Methane, CH4, reacts with oxygen to produce carbon dioxide, water, and heat. CH49) + 2O2(g) - CO2(g) + 2H2O() What is the value of AH if 5.00 g of CH4 is combusted? 157 kJ 277 kJ 445 kJ -714 kJ 1.43 104 kJ
Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2 (g) + H2O (l) ∆H = -890 kJ/mol A)Is the reaction exothermic or endothermic? B)If I combust 2 mol of methane, how much heat is absorbed or released - use the appropriate sign to indicate in your answer. C) If I combust 12.5 g of methane, how much energy in kJ is absorbed or released? Use the appropriate sign in your answer.
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.
The combustion of methane (natural gas) is given by the equation: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) ΔH = -890 kJ How much heat (in kJ) is released by the reaction of 48.5 grams of O2 with excess CH4? Remember that if heat is given off, is negative, and should be entered as such)
CREDIT Show all work for partial credit. 1) How much heat energy is released when 1000. g of methane gas (CH4) is completely reacted with excess O2 according to the following equation? (up to 8 pts) Hint: you will need to convert from g- mol energy CH& Cg)+202 (g) CO2 (g ) + 2 H20 (I)+890.4 kJ
The following thermochemical equation is for the reaction of methane(g) with oxygen(g) to form carbon dioxide(g) and water(g). CH4(g) + 2O2(g) ---> CO2(g) + 2H2O(g) H = -802 kJ When 6.37 grams of methane(g) react with excess oxygen(g), ___ kJ of energy are _________(evolved or absorbed). Once you get the answer, would it be a negative number or a positive number?
How much heat is produced if 22.2 g of octane (C8H18) is combusted according to the following reaction? 2 C8H18 (g) + 25 O2 (g) --> 16 CO2 (g) + 18 H2O (l) ΔH = -5471 kJ/mol
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