In Three Moles of Ethane C2h6 Calculate The Following

This guide explains how to calculate various properties of three moles of ethane (C2H6), including mass, volume, and energy content. The calculator on this page provides quick results, while the detailed explanation covers the underlying chemistry and physics.

Introduction

Ethane (C2H6) is a hydrocarbon with two carbon atoms and six hydrogen atoms. It's a common component of natural gas and is used in various industrial applications. Calculating properties of ethane is essential in chemistry, engineering, and environmental science.

When dealing with three moles of ethane, we can calculate several important properties using fundamental chemical principles. The molar mass of ethane is approximately 30.07 grams per mole (g/mol), which is crucial for mass calculations.

Key Properties of Ethane

Ethane has several important properties that are useful in calculations:

Molar mass: 30.07 g/mol
Density: 1.36 g/L at 20°C
Boiling point: -88.6°C
Standard molar enthalpy of combustion: -1560 kJ/mol

These properties are essential for performing calculations involving ethane. The molar mass is particularly important for mass calculations, while the density helps determine volume at standard conditions.

Calculations for Three Moles of Ethane

When working with three moles of ethane, you can calculate several important quantities:

1. Mass Calculation

The mass of three moles of ethane can be calculated using the formula:

Mass = Number of moles × Molar mass

Where:

Number of moles = 3 mol
Molar mass of ethane = 30.07 g/mol

Plugging in the values:

Mass = 3 mol × 30.07 g/mol = 90.21 g

2. Volume Calculation

The volume of three moles of ethane at standard temperature and pressure (STP) can be calculated using the ideal gas law:

Volume = (Number of moles × Gas constant × Temperature) / Pressure

Where:

Number of moles = 3 mol
Gas constant (R) = 0.0821 L·atm/(mol·K)
Temperature = 273 K (0°C)
Pressure = 1 atm

Plugging in the values:

Volume = (3 × 0.0821 × 273) / 1 = 65.2 L

3. Energy Content Calculation

The energy content of three moles of ethane can be calculated using the standard molar enthalpy of combustion:

Energy = Number of moles × Standard molar enthalpy of combustion

Where:

Number of moles = 3 mol
Standard molar enthalpy of combustion = -1560 kJ/mol

Plugging in the values:

Energy = 3 × -1560 kJ/mol = -4680 kJ

The negative sign indicates that energy is released during combustion.

Worked Examples

Example 1: Mass Calculation

Calculate the mass of 3 moles of ethane.

Solution:

Mass = Number of moles × Molar mass

Mass = 3 mol × 30.07 g/mol = 90.21 g

Example 2: Volume Calculation

Calculate the volume of 3 moles of ethane at STP.

Solution:

Volume = (Number of moles × Gas constant × Temperature) / Pressure

Volume = (3 × 0.0821 × 273) / 1 = 65.2 L

Example 3: Energy Content Calculation

Calculate the energy released when 3 moles of ethane are completely combusted.

Solution:

Energy = Number of moles × Standard molar enthalpy of combustion

Energy = 3 × -1560 kJ/mol = -4680 kJ

Frequently Asked Questions

What is the molar mass of ethane?

The molar mass of ethane (C2H6) is approximately 30.07 grams per mole (g/mol). This is calculated by summing the atomic masses of two carbon atoms and six hydrogen atoms.

How do I calculate the mass of 3 moles of ethane?

Multiply the number of moles (3) by the molar mass of ethane (30.07 g/mol). The result is 90.21 grams.

What is the standard molar enthalpy of combustion for ethane?

The standard molar enthalpy of combustion for ethane is -1560 kJ/mol. This means that burning 1 mole of ethane releases 1560 kJ of energy.

How do I calculate the volume of 3 moles of ethane at STP?

Use the ideal gas law: Volume = (Number of moles × Gas constant × Temperature) / Pressure. At STP (273 K and 1 atm), this gives 65.2 liters.

What are the key properties of ethane?

Key properties of ethane include a molar mass of 30.07 g/mol, a density of 1.36 g/L at 20°C, a boiling point of -88.6°C, and a standard molar enthalpy of combustion of -1560 kJ/mol.