SOLVED: Write a balanced equation for the combustion of CH4(g) (methane) - i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l).Given the following standard heats of formation:ΔHf° of CO2(g) is -393.5 kJ/molΔHf° of H2O(l) is -286 kJ/molΔHf° of CH4(g) is -74.8 kJ/molWhat is the standard heat of reaction (ΔH°) for the combustion reaction of CH4(g)?Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methane.(Assume standard state conditions and 2

SOLVED:Consider the balanced equation for the combustion of methane, a component of natural gas: CH4(g) 2 O2(g) ⟶CO2(g) 2 H2 O(g) Complete the table with the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as t

show the balanced chemical equation between CH4 added to O2 is equal to Co2 added to H2O