Home
Class 11
CHEMISTRY
{:("Column-I","Column-II"),("A) 1.2g of ...

`{:("Column-I","Column-II"),("A) 1.2g of carbon","P) "4.8xx10^(23)" atoms"),("B) 3g of "CO_(2),"Q) "9.034xx10^(23)" atoms"),("C) 11.2 L "CO_(2)" at S.T.P.","Q) 0.1 moles"),("D) 0.2 moles "NH_(3),"S) "9.64xx10^(24)" electrons"):}`

Text Solution

Verified by Experts

The correct Answer is:
A-R; B-S; C-Q; D-P
A) 1.2g C = 0.1 moles
B) 32g `O_(2)` implies 1 mole = `6xx10^(23)xx` atoms
`=12xx8xx10^(23)e^(-)`
C) 11.2L `CO_(2)`
`implies (1)/(2)` mole = `(1)/(2)xx6xx10^(23)xx` 3atoms
D) 0.2 moles `NH_(3)=0.2xx6xx10^(23)xx4` atoms
Promotional Banner

Similar Questions

Explore conceptually related problems

{:("Column-I","Column-II"),("A) 22.4 volume "H_(2)O_(2),"P) 11.2 litres"),("B) 32 g oxygen","Q) "9.034xx10^(23)" atoms"),("C) 11.2 L "CO_(2)" at STP","R) 2 mole"L^(-1)),("D) 1 gram equivalent hydrogen at STP","S) "9.64xx10^(24)" electron"):}

{:("Column-I","Column-II"),("A) 16g of "O_(2),"P) 1gm atom of O"),("B) Gram molar volume of "H_(2)O,"Q) 22.4 lit at STP"),("C) 18 g of "H_(2)O,"R) 18 ml"),("D) 1/2 mole "O_(2)+1" gm atom of "H_(2),"S) 11.2 lit at STP"):}

{:(,"Column-I",,"Column-II"),("A)",N_(2),"P)","40% carbon by mass"),("B)",CO,"Q)","Empirical formula "CH_(2)O),("C)",C_(6)H_(12)O_(6),"R)","Vapour density : 14"),("D)",CH_(3)COOH,"S)",14N_(A)" electrons in a mole"):}

{:(,"Column-I",,"Column-II"),("A)","One gram molecules of oxygen gas","P)","one mole of "H_(2)),("B)","Gram molar volume of "H_(2),"Q)","one mole of "O_(2)),("C)","44 gm of "CO_(2),"R)","22.4lit at STP"),("D)","18 gm water","S)",3N_(A)" atoms"):}

{:("LIST - 1","LIST - 2"),("A) 22.4 lit. at STP","1) 1 cc of "N_(2)" at STP"),("B) "18.069xx10^(23)" atoms","2) 1 mole"),("C) 108 gm. of silver","3) 4 gm. of Helium at STP"),("D) "2.69xx10^(19)" molecules","4) 2gm. of "H_(2)" at room temperature"),(,"5) 18 gm. of water"):} The correct match

{:("Column-l ","Column-II "),("(Gas) ","(Order of "T_B "Boyle Temp) (1.= min, 5 = max) "),("A)"He,"P) 3 "),("B)"CH_4 ,"Q) 5"),("C)" H_2,"R) 1 "),("D)" N_2 ,"S) 4"),("E)" NH_3 ,"T) 2 "):}

The vander waals constants a and b of a real gas are 3.6L^2 atm mol^(-2) and 0.05L mol^(-1) respectively. If 200g of gas (molecular mass 40) is placed in 10L vessel at 300K, {:("Column-I ","Column-II "),("A) Pressure correction (atm) ","P) 0.25 "),("B) Free space for the molecules to move about(L) ","Q) 0.0125 "),("C) Actual volume of the gas molecules per mole (L) ","R) 0.9 "),("D) Effective volume occupied by total gas molecules (L) ","S) 9.75 "):}

{:("Column-I","Column-II"),("A) "NH_(3),"P) EF = MF"),("B) "N_(2)H_(4),"Q) MF = "(EF)_(2)),("C) "N_(3)H,"R) Maximum percentage of nitrogen by mass "),("D) "C_(2)N_(2),"S) Least percentage of nitrogen by mass"):}