A sample of sodium bicarbonate is placed in an evacuated container at allowed to reach equilibrium. What will be the total pressure?

Complete Question

Sodium carbonate, Na2CO3(s), can be prepared by heating sodium bicarbonate, NaHCO3(s).

2NaHCO3(s) ------> Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100oC

If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100oC, what will the total gas pressure be?

The value is  

Explanation:

From the question we are told that

   The equation is  

Generally the equilibrium partial pressure is mathematically represented as

Here  

    are partial  pressures of   gases

Note: when writing the formula for equilibrium partial pressure we consider only the gas in the reaction

Let assume that    

Generally   since they are both products of the reaction

  So  

From the question we are told that

So  

=>  

=>  

=>  

So

and

So the total pressure is

=>  

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.