From the calculations performed, the free energy change for the reaction is 72 kJ/mol.
<h3>What is the equilibrium constant?</h3>
The equilibrium constant is a value that shows the extent to which reactants have been converted to products.
Given that the equation of the reaction is;
3CH4(g)→C3H8(g)+2H2(g)
Then;
PC3H8 = 0.013 atm
PH2 = 2.3×10−2 atm
PCH4 = 41 atm
Now;
ΔG = ΔG° + RTlnQ
ΔG°reaction = ΔG°products - ΔG°reactants
ΔG°reaction = [( -23.4) +2(0)] - 3(-50.8)
ΔG°reaction = 129 kJ/mol
Q = PC3H8 * PH2^2/PCH4^3
Q = 0.013 * (2.3×10−2)^2/( 41)^3
Q = 6.877 * 10^-6/68921
Q= 9.9* 10^-11
Hence;
ΔG = 129 * 10^3 + [8.314 * 298 * (ln 9.9* 10^-11 )]
ΔG = 129 * 10^3 - 57073
ΔG = 72 kJ/mol
Learn more about free energy change: brainly.com/question/14143095
Answer:
180 mg
Explanation:
For a first-order reaction, we can calculate the amount of aspirine (A) at a certain time (t) using the following expression.
where,
k: rate constant
A₀: initial amount
If we know the half-life () we can calculate the rate constant.
When t = 4 h and A₀ = 400 mg, A is:
Answer:
The signal from the deceleration sensor ignites the gas-generator mixture by an electrical impulse, creating the high-temperature condition necessary for NaN3 to decompose. The nitrogen gas that is generated then fills the airbag.
basically, the nitrogen fills the bag