Q.1
The value of $2.01 \times .011$ using significant figure is
  • .023
  • .022
  • .02211
  • .0222
Q.2
The value of $\frac {1.0042 \times .0034}{1.23}$  using significant figure is
  • .0028
  • .003
  • .002
  • .00279
Q.3
841.45 to four significant figures will be
  • 841.0
  • 841.40
  • 841.5
  • 841.4
Q.4
Which is of these zero is not significant.
  • .901
  • .011
  • .1240
  • .309
Q.5
The value of $5396 \times .045 + 325.3$ is
  • 565
  • 568.3
  • 568
  • 560
Q.6
The value of 70.3 - 1.245  using significant figure is
  • 69.1
  • 69.06
  • 69.055
  • 69.05
Q.7
The value of 10.5+1.51+2.401 using significant figure is
  • 14.5
  • 14.41
  • 14.411
  • 14.4
Q.8
Match the column
class11-chemistry-chapter-1-significant-figures-mcq-1.png
  • p -> i, q -> iii, r -> iv, s-> ii
  • p -> i, q -> iii, r -> ii, s-> iv
  • p -> ii, q -> iii, r -> ii, s-> i
  • p -> ii, q -> iii, r -> i, s-> ii
Q.9
The scientific notation for the number 0.00000060 is
  • $6 \times 10^{-7}$
  • $6.0 \times 10^{-7}$
  • $6.00 \times 10^{-7}$
  • $60 \times 10^{-8}$
Q.10
The significant figures in the number  1200 is
  • 2
  • 5
  • 3
  • 4
Q.11
70.770 to three significant figures will be
  • 70.7
  • 70.0
  • 71.0
  • 70.8
Q.12
which of these is not having 3 significant figures
  • 11100
  • 4.01
  • 1.410
  • 1.00
Q.13
12.1756  to 5 significant figures
  • 12.176
  • 12.180
  • 12.175
  • 12.170
Q.14
The value of  $1.23 \times .231$ is
  • .280
  • 0.285
  • 0.284
  • 0.28413
Q.15
The value of 415.5 + 3.64 + .238 is
  • 419.378
  • 419.4
  • 419.38
  • 420
Q.16
A solution of glucose in water is labelled as 10% w/w, The molality is
  • .74 moles/kg
  • .5 moles/kg
  • 0.62 moles/kg
  • none of these
Q.17
Which of the following terms are unit less?
  • Mole fraction
  • Formality
  • Molality
  • Molarity
Q.18
Molarity of Solution having 5 moles of solutes present in 2 L of solution is
  • 2.5 M
  • 4 M
  • .5 M
  • 2 M
Q.19
The correct expression relating molality(m) , Molarity(M), density (d) and Molar Mass(M­B) of solute is
  • $m = \frac { d - MM_B }{ M}$
  • $m = \frac {M}{d - MM_B}$
  • $m = \frac {M}{d + MM_B}$
  • $m = \frac { d + MM_B }{M }$
Q.20
The molality of the solution which contains 10 g of Cane sugar($C_{12}H_{22}O_{11}$) dissolved in 150 g of water?
  • .22 moles/kg
  • 1.1 moles/kg
  • .5 moles/kg
  • .194 moles/kg
0 h : 0 m : 1 s