Aparticular sample of pantothenic acid, a b vitamin, gives off 72.6 ml of nitrogen gas at 23 degrees c and 795 torr. what is the volume of the nitrogen at stp?

70.04 mL.

Explanation:

We can use the general law of ideal gas: V = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.  

If n is constant, and have two different values of V, P and T:

P₁V₁T₂ = P₂V₂T₁

P₁ = 795 torr, V₁ = 72.6 mL, T₁ = 23.0 °C + 273 = 296 K.

P₂ = 760 torr (standard pressure = 1 atm = 760 torr), V₂ = ??? mL,T₂ = 0.0 °C + 273 = 273 K (standard T).

∴ V₂ = P₁V₁T₂/P₂T₁ = (795 torr)(72.6 mL)(273 K)/(760 torr)(296 K) = 70.04 mL.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

b

explanation:

mitosis