Helium can be treated like an ideal gas.Helium molecules have a root-mean-square (r.m.s) speed of 730 m s-1 at a temperature of 45 oC.Calculate the r.m.s speed of the molecules at a temperature of 80 oC. Show Step 1: Write down the equation for the average translational kinetic energy: Step 2: Find the relation between cr.m.s and temperature T Since m and k are constant, <c2> is directly proportional to T <c2> ∝ T Therefore, the relation between cr.m.s and T is: Step 3: Write the equation in full where a is the constant of proportionality Step 4: Calculate the constant of proportionality from values given by rearranging for a: T = 45 oC + 273.15 = 318.15 K Step 5: Calculate cr.m.s at 80 oC by substituting the value of a and new value of T T = 80 oC + 273.15 = 353.15 K Exam TipKeep in mind this particular equation for kinetic energy is only for one molecule in the gas. If you want to find the kinetic energy for all the molecules, remember to multiply by N, the total number of molecules.You can remember the equation through the rhyme ‘Average K.E is three-halves kT’. Enter the temperature of an ideal gas into the calculator to determine the average kinetic energy of the particles in the gas.
Average Kinetic Energy FormulaThe following formula is used to calculate the average kinetic energy of a gas. K = (3/2) * (R / N) * T
To calculate the average kinetic energy of a gas, divide the gas constant by Avogadro’s number, multiply by the temperature, then again by (3/2). Average Kinetic Energy DefinitionAverage kinetic energy is defined as the average energy contained within the movement of particles of a gas. Average Kinetic Energy ExampleHow to calculate average kinetic energy?
FAQWhat is the average kinetic energy of a gas? The average kinetic energy of a gas can be calculated using the formula (3/2)*(R/N)*T for ideal gases only. According to Kinetic Molecular Theory, the average kinetic energy of gas molecules is a function only of temperature. The formula is #KE = 3/2kT# where#T#is the Kelvin temperature and#k#is Boltzmann's constant. #KE = 3/2 × 1.381 × 10⁻²³ "J·K⁻¹" × 273"K"#= 5.66 × 10⁻²¹ J For a mole of molecules, the average kinetic energy is #(5.66 × 10⁻²¹"J")/(1"molecule") × (6.022 × 10²³"molecules")/(1"mol")#= 3.41 ×10³ J/mol = 3.41 kJ/mol Answer link Related questions
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