The balanced chemical equation for the combustion of butane is:
Δ
= Σ
Δ
-Σ
Δ
= ![[{8*(-393.5kJ/mol)}+{10*(-241.82kJ/mol)}]-[{2*(-125.6kJ/mol)}+13*(0 kJ/mol)}]](https://tex.z-dn.net/?f=%5B%7B8%2A%28-393.5kJ%2Fmol%29%7D%2B%7B10%2A%28-241.82kJ%2Fmol%29%7D%5D-%5B%7B2%2A%28-125.6kJ%2Fmol%29%7D%2B13%2A%280%20kJ%2Fmol%29%7D%5D)
=[-3148kJ/mol+(-2418.2kJ/mol)]-[(-251.2kJ/mol)+0]
= -5315 kJ/mol
Calculating the enthalpy of combustion per mole of butane:
Therefore the heat of combustion per one mole butane is -2657.5 kJ/mol
Correct answer: -2657.5 kJ/mol
Ngl idk but just be a nice person and mark as brainliest please
Answer:
The average rate is 2.84 X 10⁻³ Ms⁻¹
Explanation:
Average rate = -0.5*Δ[HBr]/Δt
given;
[HBr]₁ = 0.590 M
[HBr]₂ = 0.465 M
Δ[HBr] = [HBr]₂ - [HBr]₁ = 0.465 M - 0.590 M = -0.125 M
Δt Change in time = 22.0 s
Average rate = -0.5*Δ[HBr]/Δt
Average rate = - 0.5(-0.125)/22
Average rate = 0.00284 Ms⁻¹ = 2.84 X 10⁻³ Ms⁻¹
Therefore, the average rate is 2.84 X 10⁻³ Ms⁻¹
90 miles per hour. just divide 540 by 6
The result of an exothermic reaction is released heat. According the Le Chatelier's principle, increasing<span> the </span>temperature means increasing<span> the amount of products. This means that </span><span> there will be more reactants left at equilibrium.</span>
