Mole Concept & Stoichiometry Miscellaneous Exercises — Question 42
Back to all questionsThe volume of gases A, B, C and D are in the ratio, 1 : 2 : 2 : 4 under the same conditions of temperature and pressure .
(i) Which sample of gas contains the maximum number of molecules?
(ii) If the temperature and pressure of gas A are kept constant, then what will happen to the volume of A when the number of molecules is doubled?
(iii) If this ratio of gas volume refers to the reactants and products of a reaction, which gas law is being observed?
(iv) If the volume of A is actually 5.6 dm3 at S.T.P., calculate the number of molecules in the actual Volume of D at S.T.P. (Avogadro's number is 6 × 1023).
(v) Using your answer from (iv), state the mass of D if the gas is dinitrogen oxide (N2O)
(i) Volume is directly proportional to the number of molecules, hence gas D will have maximum no. of molecules as its volume is maximum.
(ii) If number of molecules of gas A is doubled, the volume will also be doubled i.e. 2V.
(iii) Gay Lussac's Law is observed.
(iv) 1 mole contains 6 x 1023 number of molecules and occupies 22.4 lit. vol.
Given, volume of 'A' is 5.6 dm3 at s.t.p.
∴ vol. of D will be 4 × 5.6 = 22.4 lit.
No. of molecules in 22.4 lit. of D = 6 x 1023 (Avogadro no.)
(v) As D is 1 mole hence, mass of 1 mole of D (N2O) = 2(14) + 16 = 28 + 16 = 44 g
Hence, mass of N2O = 44 g