Dimethyl Propylmethane

Overview

Engineering reference data for Dimethyl Propylmethane in gases and compressed air.

Key Formulas

Ideal Gas Law

$PV = nRT$

Pressure × Volume = moles × gas constant × temperature.

Boyle's Law

$P_1 V_1 = P_2 V_2$

At constant temperature.

Charles's Law

$\frac{V_1}{T_1} = \frac{V_2}{T_2}$

At constant pressure.

Variables

Symbol	Description	Unit
$P$	Pressure	Pa
$V$	Volume	m³
$T$	Temperature	K
$R$	Gas constant	8.314 J/(mol·K)

Specific Heat Data

The following table presents the specific heat capacity of dimethyl propylmethane (C6H18) gas at constant pressure across a range of temperatures.

Unit Conversions

For the specific heat capacity values presented:

• From kJ/(kg·K):
  • To kcal/(kg·°C): multiply by 0.2389
  • To Btu/(lbm·°F): multiply by 0.2389

Example: 2.218 kJ/(kg·K) = 2.218 * 0.2389 ≈ 0.530 kcal/(kg·°C)

General Polynomial Formula

For engineering calculations, the temperature dependence of specific heat is often modeled by a polynomial. A general form for cₚ is:

$$c_p(T) = a + bT + cT^2 + dT^3$$

Where:

• $c_p(T)$ is the specific heat capacity at constant pressure (kJ/kg·K).
• $T$ is the absolute temperature (K).
• $a, b, c, d$ are empirical coefficients specific to the compound.

(Note: Coefficients for dimethyl propylmethane are not provided in the source extract. For accurate modeling, consult a chemical engineering database or thermodynamic reference.)

Interactive Charts

References

• Original Source