74. The equation for the combustion of #CH_4# (the main component of natural gas) is shown below. How much heat is produced by the complete combustion of 237 g of #CH_4#?
#CH_4 (g) + 2O_2 (g) -> CO_2 (g) + 2H_2O (g)#
#DeltaH = -"802.3 kJ/mol"#
In your case, the enthalpy change of combustion
Your strategy here will be to use the molar mass of methane to convert your sample from grams to moles
Rounded to three sig figs, the answer will be
Keep in mind that the minus sign is used to symbolize heat given off.
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The balanced equation for the combustion of CH4 is:
CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g)
The molar mass of CH4 is approximately 16.04 g/mol. The molar mass of CO2 is approximately 44.01 g/mol. The molar mass of H2O is approximately 18.02 g/mol.
The heat produced by the combustion of 1 mole of CH4 is -802.3 kJ/mol.
To find the heat produced by the combustion of 237 g of CH4, first calculate the number of moles of CH4:
moles of CH4 = mass of CH4 / molar mass of CH4
Then, use the stoichiometry of the balanced equation to find the heat produced:
moles of CH4 * (heat produced per mole of CH4)
Finally, multiply by the appropriate conversion factor to get the heat in the desired units (kJ or J).
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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