2 C2H2 + 5 O2
2 H2O + 4 CO2
what reaction type

Combustion reaction

General Formulas and Concepts:

Chemistry

Explanation:

Step 1: Define

2C₂H₂ + 5O₂ → 2H₂O + 4CO₂

Step 2: Identify

Any organic molecule reacting with oxygen to produce water and carbon dioxide is a combustion reaction.

We also see from the RxN that is is a double replacement reaction.

0.4 g

Explanation:

1) Balanced chemical equation:

2) 2C2H2 + 5 O2 → 4CO2 + 2 H2O

3) mole ratios:

2 mol C2h2 : 5 mol O2

4) Convert 0.13 g C2H2 into number of moles

n = mass in grams / molar mass

molar mass C2H2 = 2 *12g/mol + 2*1 g/mol = 26 g/mol

n = 0.13 g / 26 g/mol = 0.005 mol

5) Set the proportion with the unknown

5 mol O2             x

=

2 mol C2H2      0.005 mol C2H2

x = 0.005 mol C2H2 * 5 mol O2 / 2 mol C2H2 = 0.0125 mol O2

6) Convert 0.0125 mol O2 to grams

mass = number of moles * molar mass

molar mass of O2 = 32 g/mol

mass = 0.0125 mol * 32 g/mol = 0.4 g

0.4 g

Explanation:

Ans: Maximum amount of Fe produced = 5 moles = 280 g

The given reaction is:

Fe2O3 + 2Al → Al2O3 + 2Fe

Moles of Fe produced with respect to Fe2O3:

Based on stoichiometry, 1 mole of Fe2O3 produces 2 moles of Fe

Therefore, for the given 3 moles of Fe2O3, amount of Fe produced

= 3*2  = 6 moles

Moles of Fe produced with respect to Al:

Based on stoichiometry, 1 moles of Al produces 1 mole of Fe

Therefore, for the given 5 moles of Al, amount of Fe produced = 5 moles

Here, since Al produces less moles of Fe, Al will be the limiting reagent. Therefore, maximum moles of Fe produced = 5 moles

Atomic mass of Fe = 56 g/mol

Mass of Fe produced = 5 moles * 56 g/mol = 280 g