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question_answer1) What is the mass of water (in g) produced from 445 g of \[{{C}_{57}}\,{{H}_{110}}\,{{O}_{6}}\] in the following reaction? \[2{{C}_{57}}{{H}_{110}}{{O}_{6}}(s)+163\,\,{{O}_{2}}\to 114\,C{{O}_{2}}(g)\,+110\,{{H}_{2}}O(l)\]
question_answer2) What amount of sugar \[({{C}_{12}}{{H}_{22}}{{O}_{11}})\] (in g) is required to prepare 2L of its 0.1 M aqueous solution?
question_answer3) 5 moles of \[A{{B}_{2}}\] weigh \[125\times {{10}^{-3}}\] kg and 10 moles of \[{{A}_{2}}{{B}_{2}}\] weigh \[300\times {{10}^{-3}}\] kg. What is the sum of molar mass of \[A\,({{M}_{A}})\] and molar mass of \[B\,({{M}_{B}})\] in \[g\text{ }mo{{l}^{-1}}\text{ }\]?
question_answer4) 5.0 g of a certain element X forms 10.0 g of its oxide having the formula \[{{X}_{4}}{{O}_{6}}\]. What is the atomic mass of X in amu?
question_answer5) A 100% pure sample of a divalent metal carbonate weighing 2 g on complete thermal decomposition releases 448 cc of carbon dioxide at STP. What is the equivalent mass of the metal?
question_answer6) The specific heat of a metal is \[0.16\text{ }cal\text{ }{{g}^{-1}}\]. The equivalent mass of the metal is 20.04. What is the correct atomic mass of the metal in grams?
question_answer7) 1.500g of hydroxide of a metal gave 1.000g of its oxide on heating. What is the equivalent mass of the metal?
question_answer8) Limestone \[(CaC{{O}_{3}})\] decomposes into quicklime (CaO) on strong heating. How much quantity of limestone will be required to prepare 100 kg of quicklime?
question_answer9) 1 mole of mixture of CO and \[C{{O}_{2}}\] requires exactly 28 g KOH in solution for complete conversion of all the \[C{{O}_{2}}\] into \[{{K}_{2}}C{{O}_{3}}\]. How much amount more of KOH (in g) will be required for conversion into\[{{K}_{2}}C{{O}_{3}}\]. (If one mole of mixture is completely oxidized to \[C{{O}_{2}}\])?
question_answer10) 1 mol of \[{{N}_{2}}\] and 4 mol of \[{{H}_{2}}\] are allowed to react in a sealed container and after the reaction some water is introduced in it. The aqueous solution formed required 1 L of 1 M HCl for neutralization. Calculate the mole fraction of the gaseous product in the mixture after the reaction.
question_answer11) 6.2 g of a sample containing \[N{{a}_{2}}C{{O}_{3}},\,NaHC{{O}_{3}}\] and non- volatile inert impurity on gentle heating loses 5% of its mass due to reaction \[2\,Na\,HC{{O}_{3}}\xrightarrow{{}}N{{a}_{2}}C{{O}_{3}}+{{H}_{2}}O+C{{O}_{2}}.\] Residue is dissolved in water and formed 100 mL solution and its 10 mL portion requires 7.5 mL of 0.2 M aqueous solution of \[BaC{{l}_{2}}\] for complete precipitation of carbonates. Determine mass (in g) of \[N{{a}_{2}}C{{O}_{3}}\]in the original sample.
question_answer12) \[{{H}_{2}}{{O}_{2}}+2KI\xrightarrow{40\,(percent)\,yield}\,{{I}_{2}}\,+2KOH\] \[{{H}_{2}}{{O}_{2}}+2KMn{{O}_{4}}+3{{H}_{2}}S{{O}_{4}}\xrightarrow{50\,(percent)\,yield}\,{{K}_{2}}S{{O}_{4}}+\] \[2MnS{{O}_{4}}+3{{O}_{2}}+4{{H}_{2}}O\] 150 mL of \[{{H}_{2}}{{O}_{2}}\] sample was divided into two parts. First part was treated with KI and formed KOH required 200 mL of \[M/2\,\,{{H}_{2}}S{{O}_{4}}\] for neutralisation. Other part was treated with \[KMn{{O}_{4}}\] yielding 6.74 litre of \[{{O}_{2}}\] at 1 atm. and 273 K. Using % yield indicated find volume strength of \[{{H}_{2}}{{O}_{2}}\] sample used.
question_answer13) 5 g sample contain only \[N{{a}_{2}}C{{O}_{3}}\] and \[N{{a}_{2}}S{{O}_{4}}\]. This sample is dissolved and the volume made up to 500 mL. 25 mL of this solution neutralizes 20 mL of \[0.1\,\,M\,{{H}_{2}}\,S{{O}_{4}}.\] Calculate the percentage of \[N{{a}_{2}}S{{O}_{4}}\] in the sample.
question_answer14) A mixture of FeO and \[F{{e}_{2}}{{O}_{3}}\] is completely reacted with 100 mL of 0.25 M acidified \[KMn{{O}_{4}}\] solution. The resultant solution was then treated with Zn dust which converted \[F{{e}^{3+}}\] of the solution to\[F{{e}^{2+}}\]. The \[F{{e}^{2+}}\] required 1000 mL of \[0.10\,M\,\,{{K}_{2}}C{{r}_{2}}{{O}_{7}}\] solution. Find out the weight percentage of \[F{{e}_{2}}{{O}_{3}}\]in the mixture.
question_answer15) An impure sample of sodium oxalate \[(N{{a}_{2}}{{C}_{2}}{{O}_{4}})\]weighing 0.20 g is dissolved in aqueous solution of \[{{H}_{2}}S{{O}_{4}}\] and solution is titrated at \[70{}^\circ C\], requiring 45 mL of \[0.02\,M\,KMn{{O}_{4}}\] solution. The end point is overrun, and back titration in carried out with 10 mL of 0.1 M oxalic acid solution. Find the percentage purity of \[N{{a}_{2}}{{C}_{2}}{{O}_{4}}\] in sample.
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