Mole ConceptHard

Question

Diborane tetrachloride was treated with NaOH and the following reaction occurred.

B2Cl4 + NaOH → NaBO2 + H2O + H2 + NaCl

If 1362 ml of hydrogen gas is formed at STP, then how much B2Cl4 was consumed? (B = 11)

Options

A.9.97 g
B.9.84 g
C.0.0968 g
D.23.57 g

Solution

$B_{2}Cl_{2} + 6NaOH \rightarrow 2NaBO_{2} + 2H_{2}O + H_{2} + 4NaCl$

164 g 22700 mL at STP

∴ Mass of B2Cl4 needed =$\frac{164}{22700} \times 1362 = 9.84\text{ g}$

Create a free account to view solution

View Solution Free
Topic: Mole Concept·Practice all Mole Concept questions

More Mole Concept Questions

Silver metal in ore is dissolved by potassium cyanide solution in the presence of air by the reaction 4 Ag + 8 KCN + O2 ...A 12 g sample of CH4 and C2H4 yielded 35.2 g of CO2 on complete oxidation. What was the mean molar mass of the original ...The mineral haematite is Fe2O3. Haematite ore contains unwanted material called gangue in addition to Fe2O3. If 5 kg of ...1021 molecules are removed from 200mg of CO2. The moles of CO2 left are :...Suppose you want an acidic solution to carry out a chemical reaction with 2 moles of NaOH. Which sample of acid is the b...