Final answer:
The pressure of water vapor inside a boiler pipe at a temperature of 180°C must be higher than 1 atm, as the normal boiling point of water is 100°C at 1 atm. Estimating the exact pressure requires a vapor pressure chart or calculations based on thermodynamic principles.
Step-by-step explanation:
The question concerns the estimation of the pressure of water in a pipe, given that the temperature of the water is 180°C, and the water transitions from liquid to vapor. In chemistry, the boiling point of a substance changes with pressure.
As pressure increases, the boiling point of water also increases. The normal boiling point of water at 1 atm is 100°C. However, the question indicates that the water is boiling at 180°C, which implies that the pressure must be higher than 1 atm.
To estimate the pressure at which water will boil at 180°C, one can refer to a vapor pressure chart for water or a phase diagram for water. Vapor pressure charts show the relationship between temperature and pressure at the boiling point. The provided information suggests that at 110°C, the vapor pressure of water is about 1000 mmHg (or 1 atm).
Since we know the pressure is higher at 180°C, we can infer that the pressure at which water boils at this temperature must be significantly higher than 1 atm, though the exact value would need to be found on a more detailed vapor pressure chart or calculated using thermodynamic equations.