0.15*240=36 ml of alcohol in <span>240 ml of a 15% alcohol mixture
0.4x = </span>ml of alcohol in x ml of a 40% alcohol mixture
0.2(x+240)= ml of alcohol in (x+240) ml of a 20% alcohol mixture
0.15*240 + 0.4x = 0.2(x+240)
36+0.4x=0.2x+48
0.2x = 12
x=12/0.2=120/6=20 ml of a 40% alcohol mixture
Answer:
-133.2 kJ
Explanation:
Let's consider the following balanced equation.
4 KClO₃(s) → 3 KClO₄(s) + KCl(s)
We can calculate the standard Gibbs free energy of the reaction (ΔG°rxn) using the following expression.
ΔG°rxn = 3 mol × ΔG°f(KClO₄(s)) + 1 mol × ΔG°f(KCl(s)) - 4 mol × ΔG°f(KClO₃(s))
ΔG°rxn = 3 mol × (-303.1 kJ/mol) + 1 mol × (-409.1 kJ/mol) - 4 mol × (-296.3 kJ/mol)
ΔG°rxn = -133.2 kJ
Rubidium Chromate is the compound
I think its the mass that changes but im not sure