Question #06d81
1 Answer
Dec 25, 2017
Explanation:
- Given the
#etaCl_2# , this value can be the basis to find the#eta"C"Cl_4# through molar conversion. Refer to the provided balanced equation for the mole ratio.
#=4.0cancel(molCl_2)xx(1mol"C"Cl_4)/(2cancel(molCl_2))#
#=2mol"C"Cl_4# - Find the molar mass of the involved compound required in the problem. Relative atomic masses of the elements composing
#"C"Cl_4# are obtainable from the periodic table; i.e.,
#"Molar mass "C"Cl_4=(154 g)/(mol)# - Then, find
#m"C"Cl_4"# that can be computed as
#=2cancel(mol"C"Cl_4)xx(154g"C"Cl_4)/(1cancel(mol"C"Cl_4))#
#=308g"C"Cl_4# - Lastly, find the number of molecules of
#"C"Cl_4# . Knowing that the value in#eta"C"Cl_4=2mol# and from the relationship that#1mol"C"Cl_4=6.02xx10^23"C"Cl_4" molecules"# , the number of molecules can be computed as follows:
#=2cancel(mol"C"Cl_4)xx(6.02xx10^23"C"Cl_4" molecules")/(1cancel(mol"C"Cl_4))#
#=12.04xx10^23"C"Cl_4" molecules"# - Make sure to express the resulting value in the standard scientific notation. Knowing the fact that moving the decimal point to the left corresponds to a positive exponent (from the mnemonics LIP-Left Is Positive); that is,
#=1.2xx10^24"C"Cl_4" molecules"#
