1. Xtra Edge February 2012 - Career Point
1. Xtra Edge February 2012 - Career Point
1. Xtra Edge February 2012 - Career Point
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Step 5. 1 gram equivalent acid neutralizes 1 gram<br />
equivalent of base.<br />
∴ 0.6 + 0.36 + 0.51 V H = 3.003<br />
2SO4<br />
Solving , V H = 4 ml<br />
2SO4<br />
Step 6. 1000 ml of 1 M H2SO4 contains<br />
= 96 g SO4 2– ions<br />
96 × 17×<br />
4<br />
∴ 4ml of 17 M H2SO4 contains =<br />
1000<br />
= 6.528g SO4 2– ions<br />
9. The equilibrium constant Kp of the reaction<br />
2SO2(g) + O2(g) 2SO3(g) is 900 atm –1 at<br />
800 K. A mixture containing SO3 and O2 having<br />
initial partial pressures of 1 atm and 2 atm,<br />
respectively, is heated at constant volume to<br />
equilibrate. Calculate the pressure of each gas at<br />
800 K. [IIT- 1989]<br />
Sol. Since to start with SO2 is not present, it is expected<br />
that some of SO3 will decompose to give SO2 and<br />
O2 at equilibrium. If 2x is the partial pressure of<br />
SO3 that is decreased at equilibrium, we would<br />
have<br />
2SO2(g) + O2(g) 2SO3(g)<br />
t = 0 0 2 atm 1 atm<br />
teq 2x 2 atm + x 1 atm – 2x<br />
2<br />
( p )<br />
2<br />
SO3<br />
( 1 atm − 2x)<br />
Hence, Kp =<br />
=<br />
2<br />
2<br />
( pSO<br />
) ( p )<br />
2 O ( 2x)<br />
( 2 atm + x)<br />
2<br />
= 900 atm –1<br />
Assuming x