<span>If all chemical reactions that release free energy tend to occur spontaneously,why haven't all such reactions already occurred? One reason is that most reactions require an input of energy to get started.Before it is possible to form new chemical bonds,even bonds that contain less energy,it is first necessary to break the existing bonds,and that takes energy.The extra energy required to destabilize existing chemical bonds and initiate a chemical reaction is called activation energy.</span>
Answer:
reactants: 2 O2
products: 3 CO2, 4 NO2, 6 H2O
Explanation:
In a combustion, a combustible material, which generally is composed of C, H, O, N, and S, is combusted, that is, react with oxygen after a spark was produced; obtaining fire, heat and subproducts, including ashes and gases.
Oxygen is always one of the reactants of a combustion.
If Nitrogen was present in the combustible, NO2 (or other nitrogen oxides) will be produced.
If Carbon was present in the combustible, CO2 will be produced (also CO can be produced).
If Hydrogen was present in the combustible, H2O will be produced.
Simply, no. Except for the <span>Pyrocumulus cloud.</span>
Answer:
1177.88g of C3H8
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
C3H8 + 5O2 —> 3CO2 + 4H2O
Next we shall determine the number of mole of C3H8 required to produce 80.3 moles of CO2. This is illustrated below:
From the balanced equation above,
1 mole of C3H8 reacted to produce 3 moles of CO2.
Therefore, Xmol of C3H8 will react to produce 80.3 moles of CO2 i.e
Xmol of C3H8 = 80.3/3
Xmol of C3H8 = 26.77 moles
Finally, we shall convert 26.77 moles of C3H8 to grams.
Molar mass of C3H8 = (3x12) + (8x1) = 44g/mol
Mole of C3H8 = 26.77 moles
Mass of C3H8 =..?
Mass = mole x molar mass
Mass of C3H8 = 26.77 x 44
Mass of C3H8 = 1177.88g
Therefore, 1177.88g of C3H8 are needed for the reaction
Answer:
e. 4.1 x 10^−4
Explanation:
For the reaction;
2N2O5(g) → 4NO2(g) + O2(g)
The rate of formation is given as;
(1 / 4) Δ [O2] / Δt = (1 / 2 )Δ [N2O5] / Δt
Δ [O2] / Δt = 8.1 x 10^−4 M/s
Inserting into he equation, we have;
(1/4) (8.1 x 10^−4 ) = (1/2) (Δ [N2O5] / Δt)
2.025 x 10^−4 = (1/2) (Δ [N2O5] / Δt)
Δ [N2O5] / Δt = 2 * 2.025 x 10^−4
Δ [N2O5] / Δt = 4.1 x 10^−4
Correct option is option E.
