What pressure will cause 1.70 atm and 300.0°C to increase to 350.0°C ? Assume constant volume. Reminder : Kelvin = 273 + °C *

1.85 atm

Explanation:

Initial pressure P1 = 1.70 atm

Initial temperature T1 = 300.0°C

Convert temperature in Celsius to Kelvin i.e (273 + 300.0°C) = 573K

Final pressure P2 = ?

Final temperature T2 = 350.0°C

(273 + 350.0°C) = 623K

Mathematically, pressure law states the pressure (p) of a gas is directly proportional to the absolute temperature (T).

i.e Pressure ∝ Temperature.

P1/T1 = P2/T2

1.70 atm/573K = P2/623K

P2 = (1.70 ATM x 623K) / 573K

P2 = 1059.1/573

P2 = 1.85 atm

Thus, the 1.85 atm of pressure is required.

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey