Using this equation: CH4(g)+2O2(g)---> CO2(g)+ 2H2O(l)
What is the value of Enthalpy( triangle H) if 15.00g of O2 is reacted??
How do i set up the mole to mole ration?? with what am i comparing it too??
Make sure the equation is balanced. Is this for "so-called" standard conditions? If so, go the tables in your text and look up delta Hfo values.
delta H rxn = (delta H products) - (delta H reactants). That will give you the delta H for the reaction for 64 g oxygen. Set up a proportion to find delta H for 15 g.
To set up a mole to mole ratio, you need to compare the coefficients of the balanced chemical equation. In this case:
CH4(g) + 2O2(g) ---> CO2(g) + 2H2O(l)
The coefficients in front of each compound represent the number of moles involved in the reaction. In this equation, the coefficient of O2 is 2. So, the mole to mole ratio between CH4 and O2 is 1:2.
To find the value of Enthalpy (∆H) if 15.00g of O2 is reacted, we first need to determine the moles of O2. We'll use the molar mass of O2 to convert grams to moles.
Molar mass O2 = 32.00 g/mol
Moles of O2 = (mass of O2) / (molar mass of O2)
Moles of O2 = 15.00 g / 32.00 g/mol
After obtaining the number of moles of O2, we can use the mole to mole ratio to determine the moles of the other compounds involved in the reaction. However, in this case, we only have information about the mass of O2. We don't have any information about the moles of CH4. Therefore, we can't directly calculate the value of ∆H using this information.
To calculate the value of ∆H, we would need additional information, such as the enthalpy change per mole of the reaction (often given as ∆H per mole). This value is usually obtained from experimental data or thermodynamic tables.