Chemistry Weekly Test paper 1 class 12th
Welcome to the Class 12 Chemistry Weekly Test Paper 1! This test is specially designed to help students strengthen their understanding of key concepts in Chemistry, following the latest NCERT and CBSE syllabus. It covers important topics such as Chemical Kinetics, Electrochemistry, Solutions, and the Solid State. Practicing with this weekly test paper will not only prepare you for your board exams but also enhance your problem-solving speed and accuracy. Download the free PDF of Chemistry Weekly Test Paper 1 and start your self-assessment journey today to achieve top marks!
TEST PAPER : SOLUTION CHAPTER
CHEMISTRY TEST Full Marks : 20
CHAPTER : SOLUTION TIME : 60 Min.
Q1. Define the following terms: (i) Mole fraction (ii) Molality (iii) Molarity (iv) Mass percentage. [3]
Q2. Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL–1?
Or
Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL-1 . [3]
Q3. State Henry’s law and mention some important applications.
If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 litre of water? Assume that N2 exerts a partial pressure of 0.987 bar. Given that Henry’s law constant for N2 at 293 K is 76.48 kbar. [3]
Q4. State the Raoult’s law ?
What is meant by positive and negative deviations from Raoult’s law and how is the sign of mixH related to positive and negative deviations from Raoult’s law? [3]
Q5. What is osmotic pressure ? 200 cm3 of an aqueous solution of a protein contains 1.26 g of the protein. The osmotic pressure of such a solution at 300 K is found to be 2.57 × 10-3 bar. Calculate the molar mass of the protein [3]
Q6. Calculate the depression in the freezing point of water when 10 g of CH3CH2CHClCOOH is added to 250 g of water. Ka = 1.4 × 10–3 , Kf = 1.86 K kg mol–1
Or
Determine the amount of CaCl2 (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27° C. [2]
Q7. 45 g of ethylene glycol (C2H6O2 ) is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of the solution.
Or
1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg mol–1. Find the molar mass of the solute [3]
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SOURCE : https://ncert.nic.in/
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