314171 \(\mathrm{25 \mathrm{~g}}\) of each of the following gases are taken at \(\mathrm{27^{\circ} \mathrm{C}}\) and \(\mathrm{600 \mathrm{~mm}}\) of \(\mathrm{\mathrm{Hg}}\) pressure. Which of these will have the least volume?

314172 \(\mathrm{2.9 \mathrm{~g}}\) of a gas at \(\mathrm{95^{\circ} \mathrm{C}}\) occupied the same volume as \(\mathrm{0.184 \mathrm{~g}}\) of dihydrogen at \(\mathrm{17^{\circ} \mathrm{C}}\), at the same pressure. What is the molar mass of the gas?

314173 If 2 moles of an ideal gas at \(\mathrm{546 \mathrm{~K}}\) has volume of \(\mathrm{44.8 \mathrm{~L}}\), then what will be it's pressure?
(Given, \(\mathrm{\mathrm{R}=0.082 \mathrm{~L}}\) atm \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\) )

314174 Oxygen is present in \(\mathrm{1 \mathrm{~L}}\) flasks at a pressure of \({\rm{7}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}{\rm{\;mm}}\,\,{\rm{of}}\,\,{\rm{Hg}}\). The number of oxygen molecules in the flask at \(\mathrm{0^{\circ} \mathrm{C}}\) is

314175 \(\mathrm{\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} .1}\) mole of \(\mathrm{\mathrm{N}_{2}}\) and 4 moles of \(\mathrm{\mathrm{H}_{2}}\) are taken in \(\mathrm{15 \mathrm{~L}}\) flask at \(\mathrm{27^{\circ} \mathrm{C}}\). After complete conversion of \(\mathrm{\mathrm{N}_{2}}\) into \(\mathrm{\mathrm{NH}_{3}, 5 \mathrm{~L}}\) of water is added. Pressure set up in the flask is

314171 \(\mathrm{25 \mathrm{~g}}\) of each of the following gases are taken at \(\mathrm{27^{\circ} \mathrm{C}}\) and \(\mathrm{600 \mathrm{~mm}}\) of \(\mathrm{\mathrm{Hg}}\) pressure. Which of these will have the least volume?

314172 \(\mathrm{2.9 \mathrm{~g}}\) of a gas at \(\mathrm{95^{\circ} \mathrm{C}}\) occupied the same volume as \(\mathrm{0.184 \mathrm{~g}}\) of dihydrogen at \(\mathrm{17^{\circ} \mathrm{C}}\), at the same pressure. What is the molar mass of the gas?

314173 If 2 moles of an ideal gas at \(\mathrm{546 \mathrm{~K}}\) has volume of \(\mathrm{44.8 \mathrm{~L}}\), then what will be it's pressure?
(Given, \(\mathrm{\mathrm{R}=0.082 \mathrm{~L}}\) atm \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\) )

314174 Oxygen is present in \(\mathrm{1 \mathrm{~L}}\) flasks at a pressure of \({\rm{7}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}{\rm{\;mm}}\,\,{\rm{of}}\,\,{\rm{Hg}}\). The number of oxygen molecules in the flask at \(\mathrm{0^{\circ} \mathrm{C}}\) is

314175 \(\mathrm{\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} .1}\) mole of \(\mathrm{\mathrm{N}_{2}}\) and 4 moles of \(\mathrm{\mathrm{H}_{2}}\) are taken in \(\mathrm{15 \mathrm{~L}}\) flask at \(\mathrm{27^{\circ} \mathrm{C}}\). After complete conversion of \(\mathrm{\mathrm{N}_{2}}\) into \(\mathrm{\mathrm{NH}_{3}, 5 \mathrm{~L}}\) of water is added. Pressure set up in the flask is

314171 \(\mathrm{25 \mathrm{~g}}\) of each of the following gases are taken at \(\mathrm{27^{\circ} \mathrm{C}}\) and \(\mathrm{600 \mathrm{~mm}}\) of \(\mathrm{\mathrm{Hg}}\) pressure. Which of these will have the least volume?

314172 \(\mathrm{2.9 \mathrm{~g}}\) of a gas at \(\mathrm{95^{\circ} \mathrm{C}}\) occupied the same volume as \(\mathrm{0.184 \mathrm{~g}}\) of dihydrogen at \(\mathrm{17^{\circ} \mathrm{C}}\), at the same pressure. What is the molar mass of the gas?

314173 If 2 moles of an ideal gas at \(\mathrm{546 \mathrm{~K}}\) has volume of \(\mathrm{44.8 \mathrm{~L}}\), then what will be it's pressure?
(Given, \(\mathrm{\mathrm{R}=0.082 \mathrm{~L}}\) atm \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\) )

314174 Oxygen is present in \(\mathrm{1 \mathrm{~L}}\) flasks at a pressure of \({\rm{7}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}{\rm{\;mm}}\,\,{\rm{of}}\,\,{\rm{Hg}}\). The number of oxygen molecules in the flask at \(\mathrm{0^{\circ} \mathrm{C}}\) is

314175 \(\mathrm{\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} .1}\) mole of \(\mathrm{\mathrm{N}_{2}}\) and 4 moles of \(\mathrm{\mathrm{H}_{2}}\) are taken in \(\mathrm{15 \mathrm{~L}}\) flask at \(\mathrm{27^{\circ} \mathrm{C}}\). After complete conversion of \(\mathrm{\mathrm{N}_{2}}\) into \(\mathrm{\mathrm{NH}_{3}, 5 \mathrm{~L}}\) of water is added. Pressure set up in the flask is

314171 \(\mathrm{25 \mathrm{~g}}\) of each of the following gases are taken at \(\mathrm{27^{\circ} \mathrm{C}}\) and \(\mathrm{600 \mathrm{~mm}}\) of \(\mathrm{\mathrm{Hg}}\) pressure. Which of these will have the least volume?

314172 \(\mathrm{2.9 \mathrm{~g}}\) of a gas at \(\mathrm{95^{\circ} \mathrm{C}}\) occupied the same volume as \(\mathrm{0.184 \mathrm{~g}}\) of dihydrogen at \(\mathrm{17^{\circ} \mathrm{C}}\), at the same pressure. What is the molar mass of the gas?

314173 If 2 moles of an ideal gas at \(\mathrm{546 \mathrm{~K}}\) has volume of \(\mathrm{44.8 \mathrm{~L}}\), then what will be it's pressure?
(Given, \(\mathrm{\mathrm{R}=0.082 \mathrm{~L}}\) atm \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\) )

314174 Oxygen is present in \(\mathrm{1 \mathrm{~L}}\) flasks at a pressure of \({\rm{7}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}{\rm{\;mm}}\,\,{\rm{of}}\,\,{\rm{Hg}}\). The number of oxygen molecules in the flask at \(\mathrm{0^{\circ} \mathrm{C}}\) is

314175 \(\mathrm{\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} .1}\) mole of \(\mathrm{\mathrm{N}_{2}}\) and 4 moles of \(\mathrm{\mathrm{H}_{2}}\) are taken in \(\mathrm{15 \mathrm{~L}}\) flask at \(\mathrm{27^{\circ} \mathrm{C}}\). After complete conversion of \(\mathrm{\mathrm{N}_{2}}\) into \(\mathrm{\mathrm{NH}_{3}, 5 \mathrm{~L}}\) of water is added. Pressure set up in the flask is

314171 \(\mathrm{25 \mathrm{~g}}\) of each of the following gases are taken at \(\mathrm{27^{\circ} \mathrm{C}}\) and \(\mathrm{600 \mathrm{~mm}}\) of \(\mathrm{\mathrm{Hg}}\) pressure. Which of these will have the least volume?

314172 \(\mathrm{2.9 \mathrm{~g}}\) of a gas at \(\mathrm{95^{\circ} \mathrm{C}}\) occupied the same volume as \(\mathrm{0.184 \mathrm{~g}}\) of dihydrogen at \(\mathrm{17^{\circ} \mathrm{C}}\), at the same pressure. What is the molar mass of the gas?

314173 If 2 moles of an ideal gas at \(\mathrm{546 \mathrm{~K}}\) has volume of \(\mathrm{44.8 \mathrm{~L}}\), then what will be it's pressure?
(Given, \(\mathrm{\mathrm{R}=0.082 \mathrm{~L}}\) atm \(\mathrm{\mathrm{mol}^{-1} \mathrm{~K}^{-1}}\) )

314174 Oxygen is present in \(\mathrm{1 \mathrm{~L}}\) flasks at a pressure of \({\rm{7}}{\rm{.6 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}{\rm{\;mm}}\,\,{\rm{of}}\,\,{\rm{Hg}}\). The number of oxygen molecules in the flask at \(\mathrm{0^{\circ} \mathrm{C}}\) is

314175 \(\mathrm{\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} .1}\) mole of \(\mathrm{\mathrm{N}_{2}}\) and 4 moles of \(\mathrm{\mathrm{H}_{2}}\) are taken in \(\mathrm{15 \mathrm{~L}}\) flask at \(\mathrm{27^{\circ} \mathrm{C}}\). After complete conversion of \(\mathrm{\mathrm{N}_{2}}\) into \(\mathrm{\mathrm{NH}_{3}, 5 \mathrm{~L}}\) of water is added. Pressure set up in the flask is