Boiling Point at Altitude Calculator

Calculate Boiling Temperature at Different Elevations

Enter altitude and base boiling point to determine how boiling temperature changes with elevation. Uses atmospheric pressure models for accurate calculations.

Example Calculations

Click an example to load it into the calculator.

Water Boiling Point in Denver

Water Boiling Point in Denver

Calculate water boiling point in Denver, Colorado (1609 m above sea level). Base boiling point: 100°C.

Altitude: 1609 m

Base Boiling Point: 100 °C

Temperature Unit: Celsius (°C)

Calculation Method: Standard Atmospheric Model

Water Boiling Point on Mount Everest

Water Boiling Point on Mount Everest

Calculate water boiling point at Mount Everest base camp (5364 m above sea level). Base boiling point: 100°C.

Altitude: 5364 m

Base Boiling Point: 100 °C

Temperature Unit: Celsius (°C)

Calculation Method: Standard Atmospheric Model

Ethanol Boiling Point at High Altitude

Ethanol Boiling Point at High Altitude

Calculate ethanol boiling point at 3000 m altitude. Base boiling point: 78.37°C.

Altitude: 3000 m

Base Boiling Point: 78.37 °C

Temperature Unit: Celsius (°C)

Calculation Method: Standard Atmospheric Model

Custom Atmospheric Pressure

Custom Atmospheric Pressure

Calculate boiling point with custom atmospheric pressure of 80 kPa at 2000 m altitude. Base boiling point: 100°C.

Altitude: 2000 m

Base Boiling Point: 100 °C

Temperature Unit: Celsius (°C)

Calculation Method: Standard Atmospheric Model

Atmospheric Pressure: 80 kPa

Other Titles
Understanding Boiling Point at Altitude: A Comprehensive Guide
Master the relationship between altitude, atmospheric pressure, and boiling point with this in-depth guide.

What is Boiling Point at Altitude?

  • Definition and Basic Concepts
  • Why Boiling Point Changes with Altitude
  • Real-World Applications
Boiling point at altitude refers to the temperature at which a liquid boils when atmospheric pressure is reduced due to increased elevation above sea level. This phenomenon is crucial for understanding cooking, chemistry, and various industrial processes.
Why Boiling Point Changes with Altitude
As altitude increases, atmospheric pressure decreases. Since boiling occurs when a liquid's vapor pressure equals atmospheric pressure, lower pressure means the liquid can boil at a lower temperature. This is why water boils at temperatures below 100°C at high elevations.
Real-World Applications
Understanding boiling point changes is essential for high-altitude cooking, chemical synthesis, distillation processes, and various scientific applications where temperature control is critical.

Practical Examples:

  • Water boils at 95°C in Denver (1609 m altitude).
  • Mount Everest base camp: water boils at 84°C.
  • High-altitude cooking requires longer cooking times.

Step-by-Step Guide to Using the Calculator

  • Input Parameters
  • Calculation Methods
  • Interpreting Results
Enter the altitude above sea level, choose your preferred units, and specify the base boiling point. The calculator will determine the boiling point at the given altitude using atmospheric pressure models.
Input Parameters
Altitude can be entered in meters or feet. Temperature units include Celsius, Fahrenheit, and Kelvin. Pressure units include kPa, atm, and mmHg. The base boiling point is typically the sea-level boiling point of the substance.
Calculation Methods
Choose between standard atmospheric model (automatically calculates pressure) or custom pressure (enter known atmospheric pressure at the altitude).

Calculator Usage Examples:

  • Calculate water boiling point at 2000m altitude.
  • Determine ethanol boiling point at high elevation.
  • Use custom pressure for specific locations.

Real-World Applications of Boiling Point at Altitude

  • Cooking and Food Preparation
  • Chemical and Industrial Processes
  • Scientific Research
Understanding boiling point changes with altitude is crucial for various practical applications, from everyday cooking to complex industrial processes.
Cooking and Food Preparation
High-altitude cooking requires adjustments to cooking times and temperatures. Foods take longer to cook because water boils at lower temperatures, reducing heat transfer efficiency.
Chemical and Industrial Processes
Distillation, evaporation, and other temperature-dependent processes must be adjusted for altitude. Chemical reactions may proceed differently at different boiling points.

Application Examples:

  • Adjusting cooking times for mountain hiking.
  • Optimizing distillation processes at different elevations.
  • Understanding chemical reaction kinetics at altitude.

Common Misconceptions and Correct Methods

  • Linear vs. Non-Linear Relationships
  • Pressure vs. Temperature Effects
  • Substance-Specific Variations
Several misconceptions exist about boiling point changes with altitude, often leading to incorrect calculations and applications.
Linear vs. Non-Linear Relationships
The relationship between altitude and boiling point is not linear. The rate of change decreases with increasing altitude due to the exponential nature of atmospheric pressure decrease.
Pressure vs. Temperature Effects
It's the change in atmospheric pressure, not altitude directly, that affects boiling point. Different atmospheric conditions can result in different pressures at the same altitude.

Common Errors:

  • Assuming linear temperature decrease with altitude.
  • Ignoring atmospheric pressure variations.
  • Not considering substance-specific properties.

Mathematical Derivation and Examples

  • Atmospheric Pressure Models
  • Clausius-Clapeyron Equation
  • Practical Calculations
The calculation of boiling point at altitude involves atmospheric pressure models and thermodynamic principles that govern phase transitions.
Atmospheric Pressure Models
The International Standard Atmosphere (ISA) model provides a mathematical relationship between altitude and atmospheric pressure: P = P₀ × (1 - L×h/T₀)^(g×M/R×L), where P₀ is sea-level pressure, L is temperature lapse rate, h is altitude, T₀ is sea-level temperature, g is gravitational acceleration, M is molar mass of air, and R is the gas constant.
Clausius-Clapeyron Equation
The relationship between boiling point and pressure is described by the Clausius-Clapeyron equation: ln(P₂/P₁) = (ΔHvap/R) × (1/T₁ - 1/T₂), where ΔHvap is the heat of vaporization and T is temperature in Kelvin.

Mathematical Examples:

  • Calculate pressure at 1000m using ISA model.
  • Determine boiling point change using Clausius-Clapeyron equation.
  • Convert between different pressure units.