Calculate the Ratio of Effusion Rates of Cl2 to F2
by
Graham's Law of Effusion Calculator
Result:
The ratio of effusion rates of Cl2 to F2 will be displayed here.
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function calculateEffusionRatio() {
var molarMassCl2 = parseFloat(document.getElementById("molarMassCl2").value);
var molarMassF2 = parseFloat(document.getElementById("molarMassF2").value);
var resultDiv = document.getElementById("result");
if (isNaN(molarMassCl2) || isNaN(molarMassF2) || molarMassCl2 <= 0 || molarMassF2 <= 0) {
resultDiv.innerHTML = "Please enter valid positive molar masses for both gases.";
return;
}
// Graham's Law of Effusion states that the rate of effusion of a gas is inversely proportional
// to the square root of its molar mass.
// Rate(A) / Rate(B) = sqrt(MolarMass(B)) / sqrt(MolarMass(A))
// We want the ratio of effusion rates of Cl2 to F2, so A = Cl2 and B = F2.
// Rate(Cl2) / Rate(F2) = sqrt(MolarMass(F2)) / sqrt(MolarMass(Cl2))
var ratio = Math.sqrt(molarMassF2) / Math.sqrt(molarMassCl2);
resultDiv.innerHTML = "Ratio (Rate of Cl2 / Rate of F2): " + ratio.toFixed(4);
}
Understanding Graham's Law of Effusion
Graham's Law of Effusion is a fundamental principle in chemistry that describes the rate at which gases escape through a small opening (effusion). It states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass, assuming constant temperature and pressure. In simpler terms, lighter gases effuse (escape) faster than heavier gases.
The mathematical representation of Graham's Law is:
In this calculator, we are specifically comparing the effusion rates of Chlorine gas (Cl2) and Fluorine gas (F2). The approximate molar mass of Cl2 is 70.90 g/mol, and the approximate molar mass of F2 is 37.996 g/mol. Since F2 is significantly lighter than Cl2, we expect F2 to effuse at a higher rate.
This result indicates that for every unit of time, Chlorine gas will effuse approximately 0.732 times the amount that Fluorine gas will effuse under the same conditions. In other words, Fluorine gas effuses about 1 / 0.732 ≈ 1.366 times faster than Chlorine gas.
Graham's Law has important applications in fields like gas separation, diffusion studies, and understanding the behavior of gases at a molecular level.