A gas-filled balloon having a volume of 3.60 L at 1.15 atm and 20°C is allowed to rise to the stratosphere (about 30 km above the surface of the Earth), where the temperature and pressure are −50°C and 5.40 × 10−3 atm, respectively. Calculate the final volume of the balloon.

The new volume of the balloon will be 583.5 L

Explanation:

To calculate the volume when temperature and pressure has changed, we use the equation given by combined gas law.

The equation follows:

where,

are the initial pressure, volume and temperature of the gas

are the final pressure, volume and temperature of the gas

We are given:

Putting values in above equation, we get:

Hence, the new volume of the balloon will be 583.5 L

beta decay is the answer

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :