Hydrogen peroxide decomposes into water and oxygen - H2O2 → H2O + O2 Use the balanced equation above to calculate the following: a. What mass of oxygen is produced when 1.840 mol of H2O2 decomposes?

b. How many molecules of oxygen is this?

c. How many Liters of oxygen, measured at STP, is this? ​

Consider the following unbalanced equation for the combustion of hexane: αc6h14(g)+βo2(g)→γco2(g)+δh2o(g) part a balance the equation. give your answer as an ordered set of numbers α, β, γ, use the least possible integers for the coefficients. α α , β, γ, δ = nothing request answer part b determine how many moles of o2 are required to react completely with 5.6 moles c6h14. express your answer using two significant figures. n n = nothing mol request answer provide feedback