Question

1. From the reaction: B2H. + O2 → HBO2 + H2O
a. What mass of O2 will be needed to burn 36.1 g of B2 H.?
b. How many moles of water are produced from 19.2 g of B2H?
2. Write the balanced chemical equations of each reaction:
a. Calcium carbide (CaC2) reacts with water to form calcium hydroxide
(Ca (OH) 2) and acetylene gas (C2H2).
b. When potassium chlorate (KCIO3) is heated, it decomposes to form KCl and
oxygen gas (O2).

Answer 1

Answer:

1- balanced equation B2H6 + 3O2 → 2HBO2 + 2H2O

a.) The mass of O₂ that will be needed to burn 36.1 g B₂H, is 125.29 g.

b.) There will be 1.39 moles of water

produced from 19.2 g of B₂H⁶.

Answer 2

1. Answers to the question based on the reaction:

B2H6 + O2 => HBO2 + H2O

The balanced equation with the help of coefficients for the above reaction is:

B2H6 + 302 => 2HBO2 + 2H2O

• First, we convert the mass of B2H6 in moles:

Molecular Mass of B2H6

=> (10.811 gram/moles ×2) + (1.008 gram/moles ×6)

=>27.67 gram/mol

=>16 gram/mole ×2

: O2 molecular mass => 32 gram/mole

• Comparing the moles required in the reaction:
• We have 1 mole of B2H6 for 3 moles of O2, from the balanced equation.

(a)Now, the mass of 02

= 36.1 g B2H6 × (1 mol B2H6/27.67 g B2H6) × (3 mol O2/1 mol B2H6) × (32-gram/mol O₂)

=125.25 gram O2

(b) mass of H20

= 36.1 g B2H6×(1 mol B2H6/27.67 g B2H6) × (2 mol H2O/1 mol B2H6)

==>2.61 moles H₂0

2. Balanced equations for the reactions are:

(a) Calcium carbide (CaC2) reacts with water to form calcium hydroxide (Ca (OH) 2) and acetylene gas (C2H2).

: CaC2 + 2H2O ==> Ca(OH)2+C2H2

(b) When potassium chlorate (KCIO3) is heated, it decomposes to form KCl and

oxygen gas (O2).

: 2KClO3(s) + heat ==> 2KCl(s) + 3O2(g)