The empirical formula for the compound containing uranium and fluorine is "UF"_6". 54.2 g N2 202.2 g MgO 519.3 g FeCl3. = 238.03 + (18.998) 6 = 238.03 + 113.988 = 352.018 g/mol Hence the Molar mass of Uranium hexafluoride is 352.018 g/mol. Calculate the ratio of effusion rates for 238UF6 and 235UF6. We can set up an equation that relates the initial and final purity to the number of times the separation process is repeated: final purity = (initial purity)(separation)n, In this case, 0.990 = (0.00720)(1.0043)n, which can be rearranged to give, \[1.0043^n=\dfrac{0.990}{0.00720}=137.50 \nonumber \], \[\begin{align} n\ln(1.0043)&=\ln(137.50) \\[4pt] n &=\dfrac{\ln(137.50)}{\ln(1.0043)} \\[4pt]&=1148 \end{align} \nonumber \]. We can write the expression for the average kinetic energy of two gases with different molar masses: \[KE=\dfrac{1}{2}\dfrac{M_{\rm A}}{N_A}v_{\rm rms,A}^2=\dfrac{1}{2}\dfrac{M_{\rm B}}{N_A}v_{\rm rms,B}^2\label{10.8.2} \], Multiplying both sides by 2 and rearranging give, \[\dfrac{v_{\rm rms, B}^2}{v_{\rm rms,A}^2}=\dfrac{M_{\rm A}}{M_{\rm B}}\label{10.8.3} \], Taking the square root of both sides gives, \[\dfrac{v_{\rm rms, B}}{v_{\rm rms,A}}=\sqrt{\dfrac{M_{\rm A}}{M_{\rm B}}}\label{10.8.4} \]. "; Please enable JavaScript in order to use this website. [17], There have been several accidents involving uranium hexafluoride in the US, including a cylinder-filling accident and material release at the Sequoyah Fuels Corporation in 1986. 65 C or 338 K is the current temperature. This relationship is referred to as Grahams law, after the Scottish chemist Thomas Graham (18051869). The mean free path of a molecule is the average distance it travels between collisions. It will calculate the total mass along with the elemental composition and mass of each element in the compound. Name: Uranium Hexafluoride. Calculate the ratio of the effusion rates of, How many effusion steps are necessary to yield 99.0% pure. Enter subscripts as simple numbers. Ingmar Grenthe, Janusz Drodynski, Takeo Fujino, Edgar C. Buck. She received her MA in Environmental Science and Management from the University of California, Santa Barbara in 2016. Calculate the rms speed of a sample -butene (C4H8) at 20C. Uranium hexafluoride | UF6 - PubChem Apologies, we are having some trouble retrieving data from our servers. Formula: S3Br5. This means that if you want to find the molar mass of elements that are composed of 2 atoms, such as hydrogen, oxygen, and chlorine, then you'll have to find their relative atomic masses. There are 4 easy steps to finding the molar mass of UF6 based on its chemical formula. Yes; the answer has the correct units of moles of Fe. Let me show you the calculation to get the molar mass of Uranium hexafluoride (UF6).if(typeof ez_ad_units!='undefined'){ez_ad_units.push([[300,250],'knordslearning_com-box-4','ezslot_5',149,'0','0'])};__ez_fad_position('div-gpt-ad-knordslearning_com-box-4-0'); If you have a periodic table with you, then you can easily calculate the molar mass of Uranium hexafluoride (UF6). Examples: Fe, Au, Co, Br, C, O, N, F. You can use parenthesis () or brackets []. {"smallUrl":"https:\/\/www.wikihow.com\/images\/thumb\/6\/65\/Calculate-Molar-Mass-Step-1-Version-3.jpg\/v4-460px-Calculate-Molar-Mass-Step-1-Version-3.jpg","bigUrl":"\/images\/thumb\/6\/65\/Calculate-Molar-Mass-Step-1-Version-3.jpg\/aid1094238-v4-728px-Calculate-Molar-Mass-Step-1-Version-3.jpg","smallWidth":460,"smallHeight":345,"bigWidth":728,"bigHeight":546,"licensing":"