The ideal gas constant, r has several different values that could be used. which quantity causes these differences?
pressure
temperature
volume
moles
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Explanation:

The measure of R is always the same, but the numbers may differ depending on the units you use.

For example, in SI units, R = 8.314 Pa·m³K⁻¹mol

If your measurement uses different units, you must either convert your units to SI or use a value of R consistent with your units.

If you use bars and litres,                       R = 0.083 14   bar·L·K⁻¹mol⁻¹.

If you use kilopascals and litres,            R = 8.314        kPa·L·K⁻¹mol

If you use atmospheres and litres,        R = 0.082 06 L·atm·K⁻¹mol⁻¹.

If you use Torr and cubic centimetres, R = 62 368     Torr·cm³ K⁻¹mol⁻¹.

The only units that don't change are "K⁻¹mol⁻¹".

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 :