A 3.0 L container holds a sample of hydrogen gas at 300 K and 101.5 kPa . The pressure increases to 305 kPa and the volume remains constant. What will the temperature be?

The temperature of the Hydrogen gas at pressure is .

Explanation:

Given the volume of the Hydrogen gas remain constant.

And the initial temperature and pressure are

We need to find the temperature of the gas at

We will use the gas equation to find out that temperature. As the volume is constant we can write with pressure and temperature.

The temperature of the Hydrogen gas at pressure is .

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 :

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.