A metal crystallises in a bcc lattice. Its unit cell edge length is about 300 pm and its molar mass is about 50g mol^(-1). What would be the density of the metal ("in" g"" cm^(-3)).

A metal crystallises in a bcc lattice. Its unit cell edge length is ab

1.	A metal crystallises in a bcc lattice. Its unit cell edge length is about 300 pm and its molar mass is about 50g mol^(-1). What would be the density of the metal ("in" g"" cm^(-3)).
Answer» <html><body><p><a href="https://interviewquestions.tuteehub.com/tag/3-301577" style="font-weight:bold;" target="_blank" title="Click to know more about 3">3</a>.1<br/>6.2<br/>9.3<br/>12.4</p>Solution :`a=300"pm", Z=2`(for bcc unit cell)<br/> `M=50 g"" mol^(-1)` <br/> `"Density", rho(ZtimesM)/(N_(A)<a href="https://interviewquestions.tuteehub.com/tag/timesa-3219326" style="font-weight:bold;" target="_blank" title="Click to know more about TIMESA">TIMESA</a>^(3)times10^(-30))g""cm^(-3)`<br/> `=(2times50)/(6.02times10^(23)times(300)^(3)times10^(-30))`<br/> `=<a href="https://interviewquestions.tuteehub.com/tag/100-263808" style="font-weight:bold;" target="_blank" title="Click to know more about 100">100</a>/(6.02times27times10^(-1))`<br/> `=<a href="https://interviewquestions.tuteehub.com/tag/1000-265236" style="font-weight:bold;" target="_blank" title="Click to know more about 1000">1000</a>/(6.02times27)=6.15 g cm^(-3)`</body></html>