When 0.500 moles of boron trichloride react with 1.20 moles hydrogen gas to produce elemental boron and hydrogen chloride gas, the actual yield of boron was 66.4 % of the theoretical yield. The mass of boron obtained was _____ g.
2BCl3 + 3H2 ==> 2B + 6HCl
0.5 mol BCl2 will produce 0.5 mol B if you have all of the H2 needed.
1.20 mols H2 gas will produce 1.20 x (2 mol B/3 mols H2) = 1.20 x 2/3 = 0.8 mol B if you hadd all of the BCl3 needed.
Both answers can't be right; the correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent. In this case the LR is BCl3 and H2 is the excess reagent so you can produce 0.5 mol B as the theoretical yield. 0.5 mols x atomic mass B = estimated 5 g B. The yield is only 66.4%; therefore, you can collect only estimated 5 x 0.664 = ? g B.
Hydrogen gas is used for many purposes, including the hydrogenation of vegetable oils to make margarine. The most common industrial process for producing hydrogen is "steam reforming", in which methane gas, CH4, from natural gas
Boron has only two naturally occurring isotopes. The mass of boron-10 is 10.01294 amu and the mass of boron-11 is 11.00931 amu. Use the atomic mass of boron to calculate the relative abundance of boron-10. Atomic mass of boron is
I need to know how to figure this out, step by step... Don't assume I know anything.. Break it down for me like I'm a 5 year old... I'm really horrible at figuring out where to even begin... what steps to use.. etc.. Thank you!!
Naturally occuring boron is 80.20% boron-11 and 19.80% of some other isotopic form of boron. What must be the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass for boron?
naturally occurring boron is 80.20% boron 11 (atomic mass= 11.01amu) and 19.80% of some other isoptopic form of boron. what must the atmoci mass be be in order to account for the 10.81 amu averafe atomic mass of boron? round to
Hydrogen gas is used for many purposes, including the hydrogenation of vegetable oils to make margarine. The most common industrial process for producing hydrogen is "steam reforming," in which methane gas, CH4, from natural gas