x g of methane was burnt completely in the presence of oxygen. The liberated gases were passed into a solution containing 370 ~g of Ca ( OH )₂ . The weight of white precipitate obtained was 500 . What is the value of x (in g)? (Given : C =12 ; H =1 ; Ca =40 ; O =16 u )

Step-by-step solution

CH ₄+2 O ₂ CO ₂+2 H ₂ O Thus, 1 mole of CH ₄ gives 1 mole of CO ₂ gas. CO ₂ gas combines with Ca ( OH )₂ as :- Ca ( OH )₂+ CO ₂ CaCO ₃ + H ₂ O Thus, 1 mole of Ca ( OH )₂ gives 1 mole of CaCO ₃ precipitate or 74 ~g Ca ( OH )₂ gives 100 ~g of CaCO ₃ precipitate. Therefore, 500 ~g of precipitate would be obtained by : 74 5=370 ~g or 5 moles of Ca ( OH )₂ . Since products are formed as per the stoichiometric coefficients, there would be 5 moles of CO ₂ released in the first reaction. 5 moles of CO ₂ would be released b