For real gases, van der Waals equation is written as (p + (a n2/V2))(.V-nb.)=nRT where a and b are van der Waals constants two sets of gases are (.I.) O2,CO2,H2 and He (.II.) CH4,O2 and H2 The gases given in set-I in increasing order of b and gases given in set-II in decreasing order of a, are arranged below. Select the correct order from the following

Question

For real gases, van der Waals equation is written as (p + (a n2/V2))(.V-nb.)=nRT where a and b are van der Waals constants two sets of gases are (.I.) O2,CO2,H2 and He (.II.) CH4,O2 and H2 The gases given in set-I in increasing order of b and gases given in set-II in decreasing order of a, are arranged below. Select the correct order from the following (A) (.I.)He < H2 < CO2 < O2,(.II.)CH4>H2>O2 (B) (.I.)O2 < He < H2 < CO2,(.II.)H2>O2>CH4 (C) (.I.)H2 < He < O2 < CO2,(.II.)CH4>O2>H2 (D) (.I.)H2 < O2>He>CO2,(.II.)O2>CH4>H2

Tardigrade Admin · Accepted Answer

Van der Waals gas constant 'a' represent intermolecular force of attraction of gaseous molecules and Van der Waals gas constant 'b' represent effective size of molecules . Therefore order should be

(I) H_{2} < He < O_{2} < C O_{2}, (II) C H_{4} > O_{2} > H_{2}

$(I) He < H_{2} < C O_{2} < O_{2}, (II) C H_{4} > H_{2} > O_{2}$

$(I) O_{2} < He < H_{2} < C O_{2}, (II) H_{2} > O_{2} > C H_{4}$

$(I) H_{2} < He < O_{2} < C O_{2}, (II) C H_{4} > O_{2} > H_{2}$

$(I) H_{2} < O_{2} > He > C O_{2}, (II) O_{2} > C H_{4} > H_{2}$

Van der Waals gas constant 'a' represent intermolecular force of attraction of gaseous molecules and Van der Waals gas constant 'b' represent effective size of molecules . Therefore order should be

$(I) H_{2} < He < O_{2} < C O_{2}, (II) C H_{4} > O_{2} > H_{2}$

(I)He<H2​<CO2​<O2​,(II)CH4​>H2​>O2​

(I)O2​<He<H2​<CO2​,(II)H2​>O2​>CH4​

(I)H2​<He<O2​<CO2​,(II)CH4​>O2​>H2​

(I)H2​<O2​>He>CO2​,(II)O2​>CH4​>H2​

Van der Waals gas constant 'a' represent intermolecular force of attraction of gaseous molecules and Van der Waals gas constant 'b' represent effective size of molecules . Therefore order should be (I)H2​<He<O2​<CO2​,(II)CH4​>O2​>H2​

$(I) He < H_{2} < C O_{2} < O_{2}, (II) C H_{4} > H_{2} > O_{2}$

$(I) O_{2} < He < H_{2} < C O_{2}, (II) H_{2} > O_{2} > C H_{4}$

$(I) H_{2} < He < O_{2} < C O_{2}, (II) C H_{4} > O_{2} > H_{2}$

$(I) H_{2} < O_{2} > He > C O_{2}, (II) O_{2} > C H_{4} > H_{2}$

Van der Waals gas constant 'a' represent intermolecular force of attraction of gaseous molecules and Van der Waals gas constant 'b' represent effective size of molecules . Therefore order should be

$(I) H_{2} < He < O_{2} < C O_{2}, (II) C H_{4} > O_{2} > H_{2}$