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This section includes InterviewSolutions, each offering curated multiple-choice questions to sharpen your Class 11 knowledge and support exam preparation. Choose a topic below to get started.
1. |
How many gram of CaCO3 be decomposed to produce 20 litre of CO2at 750 torr and 27°C. |
Answer» <p><span><span><span></span></span></span></p><p><span><span><span>It is thus evident that 1 mole of CO2is obtained by decomposition of I mole of CaCO3.</span></span></span></p><p><span><span><span></span></span></span></p> | |
2. |
4 litre C2H4(g) burns in oxygen at 27°C and 1 atm to produce CO2 (g) and H20(g). Calculate the volume of CO2 formed at(a) 27°C and 1 atm,(b) 127°C and 1 atm,(c) 27°C and 2 atm. |
Answer» <p><span><span><span></span></span></span></p><p><span><span><span>(a) Under same conditions of P and T, volume of gases react in their inole ratio and produce the products in the same molar ratio. Thus, at 27°C and 1atm.</span></span></span></p><p><span><span><span></span></span></span></p><p><span><span><span></span></span></span></p> | |
3. |
A student forgot to add the reaction mixture to the round bottomed open flask at 27°C and put it on the flame. After a lapse of time, he realized his mistake, using a pyrometer he found the temperature of the flask was 477°C. What fraction of air would have been expelled out? |
Answer» <p><span>Initial mole of air in flask = n1</span></p><p><span>Temperature = 21 + 273 = 300 K</span></p><p><span>Final mole of air in flask = n2</span></p><p><span>Temperature = 477 + 273 = 750 K</span></p><p><span>The volume and pressure remains constant, thus, n1T1= n2T2</span></p><p><span>n2= n1x 300/750 = 2/5 n1</span></p><p><span>Thus, air expelled out on heating = n1- n2= n1- (2/5) n1= 3/5 n1</span></p><p><span>orfraction of air expelled = 3/5.</span></p> | |
4. |
Through the two ends of a glass tube of length 200 cmhydrogen chloride gas and ammonia are allowed to enter. At what distance ammonium chloride will first appear? |
Answer» <p><span><span><span></span></span></span></p><p><span><span><span>Let a cm from HClend white fumes of NH4Clare noticed.</span></span></span></p><p><span><span><span>From Graham's law</span></span></span></p><p><span><span><span></span></span></span></p><p></p> | |
5. |
For 10 minutes each, at 27°C, from two identical holes nitrogen and an unknown gas are leaked into a common vessel of 3 litre capacity. The resulting pressure is 4.18 bar and the mixture contains 0.4 mole of nitrogen. What is the molar mass of the unknown gas? |
Answer» <p><span><span><span></span></span></span></p><p><span><span><span>For the diffusion of both gases for 10 minutes under identical conditions</span></span></span></p><p><span><span><span></span></span></span></p><p><span><span><span></span></span></span></p> | |
6. |
6.0 g He and 12.0 g Ne molecules both having average velocity of 4 x 10^2 ms-1 are mixed. Calculate kinetic energy per mole of the mixture. |
Answer» <p><span><span><span>For He:</span></span></span></p><p><span><span><span></span></span></span></p><p><span><span><span>For Ne:</span></span></span></p><p><span><span><span></span></span></span></p><p><span><span><span></span></span></span></p><p></p> | |