A fixed mass of a gas occupies a volume of 150 cm 3 at a fixed temperature and a pressure of 1 atmosphere. What volume will the gas occupy at that temperature and at a pressure of 1.5 atmosphere?

Given, P 1 = 1 atm V 1 = 150 cm 3 P 2 = 1 . 5 atm V 2 = ? We know that PV = nRT The temperature is fixed, therefore, P 1 V 1 = P 2 V 2 V 2 = P 1 V 1 P 2 = 1 × 150 1 . 5 = 100 cm 3

State Avogadro's law. At a certain fixed temperature and pressure the molar volumes ( V / n ) of the real gases are nearly equal and at STP the limit is 22 . 4 Lmol - 1 . How Avogadro's law can be arrived at from this information obtained from experiments?

Avogadro’s law is a gas law which states that the total number of atoms/molecules of a gas (i.e. the amount of gaseous substance) is directly proportional to the volume occupied by the gas at constant temperature and pressure. At a certain fixed temperature and pressure the molar volumes ( V / n ) of the real gases are nearly equal and at STP the limit is 22 . 4 Lmol - 1 . Then, V 1 n 1 = V 2 n 2 V 1 n 1 = V 2 n 2 = K , where K is Avogadro constant. Which means that V α n As number of moles increases, volume increases.

A fixed mass of a gas occupies a volume of 520 cm 3 at - 13 ° C temperature. Keeping the pressure unchanged, when the gas is heated the volume of the gas increases to 700 cm 3 . What is the final temperature of the gas in degree celsius?

By ideal gas equation, PV = nRT As pressure is unchanged, we can write, V 1 T 1 = V 2 T 2 Given, V 1 = 520 cm 3 , V 2 = 700 cm 3 T 1 = ( 273 - 13 ) = 260 K 520 260 = 700 T 2 T 2 = 350 K The final temperature in degree Celsius ( 350 - 273 ) = 77 ° C

Find out the ratio of the volumes occupied by 32 g O , and 44 g CO 2 , gases at 27 ° C temperature and 700 mmHg pressure. ( C = 12 , O = 16 )

We know that the volume of gas does not depend on molar mass/molecular weight of the gas. It simply depends on number of moles, temperature and pressure. Molar mass of oxygen = 32 g = 1 mol Molar mass of carbon dioxide = 12 + 32 = 44 g = 1 mol Number of moles is equal in both cases, therefore, V O 2 V CO 2 = 1 1 , as temperature, pressure both are same. Hence, the ratio of volumes is 1 : 1

Under constant pressure, at what temperature in a degree Celsius, the volume of an ideal gas will be zero according to Charles law?

According to Charles law, the volume of the gas rises by 1 273 times its initial volume at 0 ° C with every degree increase in temperature at constant. V = V o + t 273 V o ; where V o is the initial volume and V is the final volume. If t = - 273 ; V = V o 1 - 273 273 ; then V ⇒ 0 Hence, at - 273 ° C , the volume of the gas becomes zero.

What is the unit of volume expansion coefficient?

The SI unit of coefficient of volume expansion is ° C - 1 . Volume expansion is defined as the increase in the volume of the solid on heating. Change in temperature ∆ t the change in volume of a solid.