CH4 (g) + 2 O2 (g) --> CO2 (g) + 2 H2O (g), (triangle)H rxn =-802.3 kj
How much heat is produced by the complete combustion of 237 g of CH4?
You know you get 802.3 kJ for burning 16 g CH4 and you know that from the question. All you need to do is to convert that to (it's just a proportion) to 237 and not 16 g CH4.
heat produced is 802.3 kJ x (237/16) = ?
11884.06875
To calculate the amount of heat produced by the complete combustion of 237g of CH4 (methane), we will use the given enthalpy of the reaction and the stoichiometry of the reaction.
The given reaction is:
CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
From the balanced equation, we can see that one mole of CH4 reacts to produce one mole of CO2 and two moles of H2O.
1 mole of CH4 → -802.3 kJ of heat energy
To calculate the amount of heat produced by the complete combustion of 237g of CH4, we will use the molar mass of CH4 to convert grams to moles.
Molar mass of CH4:
C = 12.01 g/mol
H = 1.01 g/mol (4 hydrogen atoms in CH4)
Total molar mass of CH4:
12.01 g/mol + (4 * 1.01 g/mol) = 16.04 g/mol
Now, we can calculate the number of moles of CH4 in 237g:
Number of moles = mass / molar mass
Number of moles = 237g / 16.04 g/mol
Number of moles = 14.77 mol
Now, we multiply the number of moles of CH4 by the heat energy produced per mole:
Heat energy = number of moles * ΔH
Heat energy = 14.77 mol * -802.3 kJ/mol
Finally, we can calculate the heat produced:
Heat energy = -11857.771 kJ
Therefore, the complete combustion of 237g of CH4 would produce approximately -11857.771 kJ of heat energy.
To determine the amount of heat produced by the complete combustion of 237 g of CH4, you need to use the given information about the heat of reaction (∆Hrxn).
The first step is to calculate the molar mass of CH4 (methane), which consists of one carbon (C) atom with a molar mass of 12.01 g/mol and four hydrogen (H) atoms with a molar mass of 1.01 g/mol.
Molar mass of CH4 = (1 x 12.01 g/mol) + (4 x 1.01 g/mol) = 16.05 g/mol
Since the balanced chemical equation states that CH4 reacts with 2 moles of O2, the molar ratio is 1:2. Therefore, one mole of CH4 produces ∆Hrxn of -802.3 kJ.
Now, we can use this information to calculate the amount of heat produced by the combustion of 237 g of CH4.
First, convert the mass of CH4 to moles by using the molar mass:
Moles of CH4 = mass / molar mass = 237 g / 16.05 g/mol = 14.75 mol
Since the molar ratio of CH4 to ∆Hrxn is 1:∆Hrxn, you can set up a proportion to find the heat produced:
14.75 mol CH4 / 1 * -802.3 kJ / 1 mol CH4 = -11,823.925 kJ
Therefore, the complete combustion of 237 g of CH4 would produce approximately -11,823.925 kJ of heat. Note that the negative sign indicates that the reaction is exothermic and releases heat.