314202 Consider the following statements.
I. One mole of each gas at standard temperature and pressure will have same volume.
II. At STP, molar volume of an ideal gas or a combination of ideal gases is \(\mathrm{22.7 \mathrm{~L} \mathrm{~mol}^{-1}}\).
III. The combined gas law is given by
\(\rm{\dfrac{p_{1} V_{1}}{T_{1}}=\dfrac{p_{2} V_{2}}{T_{2}}}\).
IV. In ideal gas equation, \(\mathrm{\mathrm{R}}\) is called universal gas constant
Choose the correct statement and select the correct option.

314203 The density of a gas is \(1.964 \mathrm{~g} \mathrm{dm}^{-3}\) at \(273 \mathrm{~K}\) and \(76\;{\rm{cm}}\,{\rm{Hg}}\). The gas is

314204 The pressure and temperature of \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) of carbon dioxide gas are doubled. Then, volume of carbon dioxide gas would be

314205 By the ideal gas law, the pressure of \({\rm{0}}.{\rm{60}}\;{\rm{mole}}\,{\rm{N}}{{\rm{H}}_{\rm{3}}}\,{\rm{gas}}\,{\rm{in}}\,{\rm{a}}\,{\rm{3}}{\rm{.00}}\;{\rm{L}}\,{\rm{vessel}}\,{\mkern 1mu} {\rm{at\, 25^\circ C}}\,{\rm{is}}\)

314206 For a given mass of gas, if pressure is reduced to half and the absolute temperature is increased two times, then the volume would be become

314202 Consider the following statements.
I. One mole of each gas at standard temperature and pressure will have same volume.
II. At STP, molar volume of an ideal gas or a combination of ideal gases is \(\mathrm{22.7 \mathrm{~L} \mathrm{~mol}^{-1}}\).
III. The combined gas law is given by
\(\rm{\dfrac{p_{1} V_{1}}{T_{1}}=\dfrac{p_{2} V_{2}}{T_{2}}}\).
IV. In ideal gas equation, \(\mathrm{\mathrm{R}}\) is called universal gas constant
Choose the correct statement and select the correct option.

314203 The density of a gas is \(1.964 \mathrm{~g} \mathrm{dm}^{-3}\) at \(273 \mathrm{~K}\) and \(76\;{\rm{cm}}\,{\rm{Hg}}\). The gas is

314204 The pressure and temperature of \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) of carbon dioxide gas are doubled. Then, volume of carbon dioxide gas would be

314205 By the ideal gas law, the pressure of \({\rm{0}}.{\rm{60}}\;{\rm{mole}}\,{\rm{N}}{{\rm{H}}_{\rm{3}}}\,{\rm{gas}}\,{\rm{in}}\,{\rm{a}}\,{\rm{3}}{\rm{.00}}\;{\rm{L}}\,{\rm{vessel}}\,{\mkern 1mu} {\rm{at\, 25^\circ C}}\,{\rm{is}}\)

314206 For a given mass of gas, if pressure is reduced to half and the absolute temperature is increased two times, then the volume would be become

314202 Consider the following statements.
I. One mole of each gas at standard temperature and pressure will have same volume.
II. At STP, molar volume of an ideal gas or a combination of ideal gases is \(\mathrm{22.7 \mathrm{~L} \mathrm{~mol}^{-1}}\).
III. The combined gas law is given by
\(\rm{\dfrac{p_{1} V_{1}}{T_{1}}=\dfrac{p_{2} V_{2}}{T_{2}}}\).
IV. In ideal gas equation, \(\mathrm{\mathrm{R}}\) is called universal gas constant
Choose the correct statement and select the correct option.

314203 The density of a gas is \(1.964 \mathrm{~g} \mathrm{dm}^{-3}\) at \(273 \mathrm{~K}\) and \(76\;{\rm{cm}}\,{\rm{Hg}}\). The gas is

314204 The pressure and temperature of \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) of carbon dioxide gas are doubled. Then, volume of carbon dioxide gas would be

314205 By the ideal gas law, the pressure of \({\rm{0}}.{\rm{60}}\;{\rm{mole}}\,{\rm{N}}{{\rm{H}}_{\rm{3}}}\,{\rm{gas}}\,{\rm{in}}\,{\rm{a}}\,{\rm{3}}{\rm{.00}}\;{\rm{L}}\,{\rm{vessel}}\,{\mkern 1mu} {\rm{at\, 25^\circ C}}\,{\rm{is}}\)

314206 For a given mass of gas, if pressure is reduced to half and the absolute temperature is increased two times, then the volume would be become

314202 Consider the following statements.
I. One mole of each gas at standard temperature and pressure will have same volume.
II. At STP, molar volume of an ideal gas or a combination of ideal gases is \(\mathrm{22.7 \mathrm{~L} \mathrm{~mol}^{-1}}\).
III. The combined gas law is given by
\(\rm{\dfrac{p_{1} V_{1}}{T_{1}}=\dfrac{p_{2} V_{2}}{T_{2}}}\).
IV. In ideal gas equation, \(\mathrm{\mathrm{R}}\) is called universal gas constant
Choose the correct statement and select the correct option.

314203 The density of a gas is \(1.964 \mathrm{~g} \mathrm{dm}^{-3}\) at \(273 \mathrm{~K}\) and \(76\;{\rm{cm}}\,{\rm{Hg}}\). The gas is

314204 The pressure and temperature of \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) of carbon dioxide gas are doubled. Then, volume of carbon dioxide gas would be

314205 By the ideal gas law, the pressure of \({\rm{0}}.{\rm{60}}\;{\rm{mole}}\,{\rm{N}}{{\rm{H}}_{\rm{3}}}\,{\rm{gas}}\,{\rm{in}}\,{\rm{a}}\,{\rm{3}}{\rm{.00}}\;{\rm{L}}\,{\rm{vessel}}\,{\mkern 1mu} {\rm{at\, 25^\circ C}}\,{\rm{is}}\)

314206 For a given mass of gas, if pressure is reduced to half and the absolute temperature is increased two times, then the volume would be become

314202 Consider the following statements.
I. One mole of each gas at standard temperature and pressure will have same volume.
II. At STP, molar volume of an ideal gas or a combination of ideal gases is \(\mathrm{22.7 \mathrm{~L} \mathrm{~mol}^{-1}}\).
III. The combined gas law is given by
\(\rm{\dfrac{p_{1} V_{1}}{T_{1}}=\dfrac{p_{2} V_{2}}{T_{2}}}\).
IV. In ideal gas equation, \(\mathrm{\mathrm{R}}\) is called universal gas constant
Choose the correct statement and select the correct option.

314203 The density of a gas is \(1.964 \mathrm{~g} \mathrm{dm}^{-3}\) at \(273 \mathrm{~K}\) and \(76\;{\rm{cm}}\,{\rm{Hg}}\). The gas is

314204 The pressure and temperature of \({\rm{4}}\,{\rm{d}}{{\rm{m}}^{\rm{3}}}\) of carbon dioxide gas are doubled. Then, volume of carbon dioxide gas would be

314205 By the ideal gas law, the pressure of \({\rm{0}}.{\rm{60}}\;{\rm{mole}}\,{\rm{N}}{{\rm{H}}_{\rm{3}}}\,{\rm{gas}}\,{\rm{in}}\,{\rm{a}}\,{\rm{3}}{\rm{.00}}\;{\rm{L}}\,{\rm{vessel}}\,{\mkern 1mu} {\rm{at\, 25^\circ C}}\,{\rm{is}}\)

314206 For a given mass of gas, if pressure is reduced to half and the absolute temperature is increased two times, then the volume would be become