What is the product of pressure and volume of 2g of hydrogen at STP? H = 1

Given, Mass of hydrogen = 2 g Molecular weight of hydrogen = 2 The value of the universal gas constant R at STP = 8 . 314 Jmol − 1 K − 1 From ideal gas equation: PV = nRT = m M RT PV = 2 2 × 8 . 314 × 273 PV = 2 . 269 × 10 3 m 3 . mmHg

Under constant pressure, at what temperature in a degree Celsius, the volume of an ideal gas will be zero according to Charles law?

According to Charles law, the volume of the gas rises by 1 273 times its initial volume at 0 ° C with every degree increase in temperature at constant. V = V o + t 273 V o ; where V o is the initial volume and V is the final volume. If t = - 273 ; V = V o 1 - 273 273 ; then V ⇒ 0 Hence, at - 273 ° C , the volume of the gas becomes zero.

Establish the ideal gas equation on the basis of Boyle’s law, Charles law and Avogadro’s law.

Boyle's law, Charles' law and Avogadro's law can be combined in a single equation called ideal gas equation. This equation can be derived as given below: According to Boyle's law, V ∝ 1 P (at constant T and n )---------(i) According to Charles' law, V ∝ T (at constant P ) and ----------(ii) According to Avogadro's law, V ∝ n (at constant P and T )----------(iii), where n is the number of moles of the gas. On combining equations (i), (ii) and (iii) we get, V ∝ 1 P × T × n , V = R × nT P ----(iv), where, R is proportionality constant and is found to be independent of the nature of the gas and depends only on the amount of the gas taken. For one mole of any gas, the value of R is the same. Hence, R is called 'universal gas constant'. On rearranging the equation (iv), we get PV = nRT , this is called an ideal gas equation.