Balanced chemical equation is:
2 LiHCO3 + H2SO4 ---> Li2SO4 +
2 mol of LiHCO3 reacts with 1 mol of H2SO4
for 4.5 mol of LiHCO3, 2.25 mol of H2SO4 is required
But we have 8.5 mol of H2SO4
so, LiHCO3 is limiting reagent
According to balanced equation
mol of H2SO4 reacted = (1/2)* moles of LiHCO3
= (1/2)*4.5
= 2.25 mol
mol of H2SO4 remaining = mol initially present - mol reacted
mol of H2SO4 remaining = 8.5 - 2.25
mol of H2SO4 remaining = 6.25 mol
Molar mass of H2SO4 = 98.08 g/mol
use:
mass of H2SO4,
m = number of mol * molar mass
= 6.25 mol * 98.08 g/mol
= 613 g
Answer: d
b0.795 g fon . Calculate the mass of excess reactant remaining after 4.50 mol of LiHCO3...
molar 7. How many grams of CO 28.01 /mol) must be bumed to produce 225 kJ of heat urma 2006 +020 200260 AH = -566 kJ c) 2238 ite a) 0.398 8 b) 0.795 g c) 2.52 g d) 11.1 g 3. Calculate the mass of excess reactant remaining after 4.50 mol of LHCO (67.96 R/mol) and 8.50 mol of H2504 (98.08 g/mol) reacted according to the equation shown below. 2LHCO3 + H2SO4 - Li2SO4 + 2H20 + 2002 e)...
Determine the quantity of excess reactant (in moles) that remains after a reaction if 0.50 mol of BCI3 and 2.1 mol of H20 are reacted according to the following balanced reaction. Assume that the reaction goes to completion BCI3(g) +3 H20() H3BO3(s)+3 HCl(g) 1.6 mol 0.60 mol 1.5 mol 2.1 mol 0.2