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^{o}C, R = 8.314 J mol^{-1 }K^{-1}is :^{-3}and pressure 1.2 * 10^{5}N m^{-2}is :^{-12}g and at temperature 27^{o}C is :^{-2}L mol^{-1}. H owclose the nuclei of the two molecules can come together .^{o}C is nearby :_{2}is equal to that of neon at 300 K is :_{2}has the same R.M.S. speed to that of O_{2}at S.T.P. is/are :^{-1}K^{-1}_{2}& other with 1 kg H_{2}. The N_{2}balloon leaks to a pressure of 1/2 atm in one hour. How long will it take for H_{2}balloon to leaks to a pressure of1atm. 2

a) 273K,2 bar

b)273 C, 0.5 atm

c. 273 c and 2 atm

d. 546 c , 1.5 atm

_{2}be 1.6 times the rate of diffusion of So_{2}at 27 degrees c^{-15}kg at 300 kWhich of following statements justifies the use of Boyles law?

A. Gases are compressible.

B. Gases expand on heating.

C. Pressure of a gas is independent of its temperature.

D. For a given mass of a gas, pressure and volume remain the same.

I CANT UNDERSTAND PARTIAL PRESSUREOR HOW P IS INVERSLY PROPORTION TO VOLUME I CANT UNDERSTAND

According to kinetic molecular theory of gases, PV=mnc^2+3 where c=rms velocity of the gas. Now if we create a condition where the rms velocity gets converted to the speed of light then what would happen to this gas? (assumed condition:we can create very high temperatures in laboratory i.e.upto 1,85,25,727k)Explain this question. From where did the temperature come to be 300K. Why R is taken in ergs not in joule? What is deg written after ergs in units of R ??

^{-3}_{}Options:_{1}= P_{2}> P_{3}_{3}= P_{2}> P_{1}_{1}> P_{2}> P_{3}_{3}> P_{2}> P_{1}_{2}will be tripled and K.E will be 4 times .please solve this question step by step.