https://ejercicios-fyq.com/ Ejercicios Resueltos, Situaciones de aprendizaje y VÍDEOS de Física y Química para Secundaria y Bachillerato es SPIP - www.spip.net https://ejercicios-fyq.com/local/cache-vignettes/L144xH25/siteon0-da713.png?1758361862 https://ejercicios-fyq.com/ 25 144 https://ejercicios-fyq.com/Application-of-Graham-s-law-hydrogen-diffusion-rate-8308 https://ejercicios-fyq.com/Application-of-Graham-s-law-hydrogen-diffusion-rate-8308 2024-09-12T04:06:10Z text/html es F_y_Q Gas laws Graham's law SOLVED <p>Determine the diffusion rate of hydrogen, knowing that the diffusion rate of oxygen is 2 minutes.</p> - <a href="https://ejercicios-fyq.com/Matter-and-gas-laws" rel="directory">Matter and gas laws</a> / <a href="https://ejercicios-fyq.com/Gas-laws" rel="tag">Gas laws</a>, <a href="https://ejercicios-fyq.com/Graham-s-law" rel="tag">Graham's law</a>, <a href="https://ejercicios-fyq.com/SOLVED" rel="tag">SOLVED</a> <div class='rss_texte'><p>Determine the diffusion rate of hydrogen, knowing that the diffusion rate of oxygen is 2 minutes.</p></div> <hr /> <div <div class='rss_ps'><p>Graham's law relates the diffusion rates of two gases to their molecular masses. If the gases are A and B, the relationship is: <br/> <br/> <img src='https://ejercicios-fyq.com/local/cache-TeX/4cf3fe04d22fc72e2d726e95ac2bdc33.png' style="vertical-align:middle;" width="126" height="65" alt="\color[RGB]{2,112,20}{\bm{\frac{v_A}{v_B} = \sqrt{\frac{M_B}{M_A}}}}" title="\color[RGB]{2,112,20}{\bm{\frac{v_A}{v_B} = \sqrt{\frac{M_B}{M_A}}}}" /> <br/> <br/> For hydrogen and oxygen, both being diatomic, the molecular masses are: <br/> <br/> <img src='https://ejercicios-fyq.com/local/cache-TeX/fa228ad48fcef891303029aae15bb4aa.png' style="vertical-align:middle;" width="179" height="52" alt="\left \ce{H2}: 2\cdot 1 = {\color[RGB]{0,112,192}{\bf 2\ u}} \atop \ce{O2}: 2\cdot 16 = {\color[RGB]{0,112,192}{\bf 32\ u}} \right \}" title="\left \ce{H2}: 2\cdot 1 = {\color[RGB]{0,112,192}{\bf 2\ u}} \atop \ce{O2}: 2\cdot 16 = {\color[RGB]{0,112,192}{\bf 32\ u}} \right \}" /> <br/> <br/> The relationship between their diffusion rates will be: <br/> <br/> <img src='https://ejercicios-fyq.com/local/cache-TeX/d7383bc419efafca3c82287879aa12d2.png' style="vertical-align:middle;" width="236" height="55" alt="\frac{v_{\ce{H_2}}}{v_{\ce{O_2}}}= \sqrt{\frac{32\ \cancel{u}}{2\ \cancel{u}}} = \sqrt{16} = \color[RGB]{0,112,192}{\bf 4}" title="\frac{v_{\ce{H_2}}}{v_{\ce{O_2}}}= \sqrt{\frac{32\ \cancel{u}}{2\ \cancel{u}}} = \sqrt{16} = \color[RGB]{0,112,192}{\bf 4}" /> <br/> <br/> This means hydrogen diffuses four times faster than oxygen, so <b>the diffusion rate of hydrogen will be 0.5 minutes</b>, or 30 seconds</b>.</math></p></div>