10g of oxygen was introduced in an evacuated container of 5 dm3 volume at 27 C calculate pressure of gas in Nm-2
A given mass of a gas occupies volume of 2.5dm3 at NTP. calculate the change in volume of gas at the same temperature if pressure of a gas is changed to 1.04*105Nm-2
state and explain Boyles's law with the help of suitable example
In the chemical reaction : N2 = 3H2 2NH3 At equilibrium point, state whether
[1] Equal volumes of N2 and H2 are reacting
[2] Equal masses of N2 and H2 are reacting
[3] The reaction has stopped
[4] The same amount of ammonia is formed as is decomposed into N2 and H2
10g of oxygen was introduced in an evacuated container of 5 dm3 volume at 27 C calculate pressure of gas in Nm-2
A) 15 atm and 200 K
B) 1 atm and 273 K
C) 0.5 atm and 500 K
D) 15 atm and 500 K
A given mass of a gas occupies volume of 2.5dm3 at NTP. calculate the change in volume of gas at the same temperature if pressure of a gas is changed to 1.04*105Nm-2
(a) = 2
(b) = 1
(c) = 4
(d) = 3
state and explain Boyles's law with the help of suitable example
In the chemical reaction : N2 = 3H2 2NH3 At equilibrium point, state whether
[1] Equal volumes of N2 and H2 are reacting
[2] Equal masses of N2 and H2 are reacting
[3] The reaction has stopped
[4] The same amount of ammonia is formed as is decomposed into N2 and H2
(A) 3.9 × 104 (B) 2.5 × 104 (C) 1.0 × 104 (D) 1.84 × 105
Q.11 (S) 0.5 mole each of two ideal gases A and B ( = 3 R) are taken in a container and expanded reversibly and adiabatically, during this process temperature of gaseous mixture decreased from 350 K and 250 K. Find H (in cal/mol) for the process :
(a) - 100 R
(b) - 137.5 R
(c) - 375 R
(d) None of these