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Chapter 1: Problem 41
Calculate the molarity of a solution obtained by mixing \(250 \mathrm{ml}\) of \(0.5 \mathrm{M}\) HCl with \(750 \mathrm{ml}\) of \(2 \mathrm{M}\) HCl. (a) \(1.8\) (b) \(2.0\) (c) \(1.6\) (d) \(0.8\)
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Match the entries given in Column A with appropriate ones in Column \(B\). $$ \begin{array}{|l|l|l|} \hline \begin{array}{l} \text { A. Empirical formula of } \\ \text { glucose } \end{array} & \text { () } & \begin{array}{l} \text { a. Less intermolecular } \\ \text { forces } \end{array} \\ \hline \begin{array}{l} \text { B. Percentage of carbon } \\ \text { in methane } \end{array} & \text { () } & \text { b. } 75 \% \\ \hline \text { C. Ideal gas } & \text { () } & \text { c. } 17.6 \% \\ \hline \text { D. High critical } & \text { () } & \begin{array}{l} \text { d. } \text { Large } \\ \text { intermolecular } \\ \text { forces of attraction } \end{array} \\ \hline \begin{array}{l} \text { E. Percentage of } \\ \text { hydrogen in } \\ \text { ammonia } \end{array} & \text { () } & \text { e. } \mathrm{CH}_{2} \mathrm{O} \\ \hline \begin{array}{l} \text { F. } \text { Empirical formula of } \\ \text { oxalic acid } \end{array} & \text { () } & \text { f. } \mathrm{CHO}_{2} \\ \hline \end{array} $$
\(\mathrm{KMnO}_{4}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{FeSO}_{4} \rightarrow \mathrm{K}_{2} \mathrm{SO}_{4}+\mathrm{MnSO}_{4}+\) \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}+\mathrm{H}_{2} \mathrm{O}\) Coefficients of sulphuric acid and ferric sulphate in the balanced equation of above reaction are respectively (a) 8,4 (b) 5,8 (c) 4,3 (d) 8,5
Fill in the blanks. Pressure exerted by water vapour in moist gas is called
Fill in the blanks. The ratio of the volumes of \(11 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(28 \mathrm{~g}\) of \(\mathrm{CO}\) at \(\mathrm{STP}\) is
Select the correct alternative from the given choices. \(20 \mathrm{cc}\) of a hydrocarbon on complete combustion gave \(80 \mathrm{cc}\) of \(\mathrm{CO}_{2}\) and \(100 \mathrm{cc}\) of \(\mathrm{H}_{2} \mathrm{O}\) at \(\mathrm{STP}\). The empirical formula of that compound is (a) \(\mathrm{C}_{2} \mathrm{H}_{5}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{8}\) (d) \(\mathrm{C}_{4} \mathrm{H}_{10}\)
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