0.1 M solution of each of $N H_{3}$ and $N H_{4} C l$ are added to prepare a buffer of 1 litre solution. If 0.01 mole of HCl is added (assuming no volume change). The concentrations of $N H_{3}$ and $N H_{4} C l$ are

Q. A mixture of

2

moles of

H_{2}

3

moles of

N H_{3}

4

moles of

C O_{2}

and

5

moles of

N_{2}

exerts a total pressure of

798

torr. What is the partial pressure of

C O_{2}

gas ?

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HCl(g)+NH3(g)−NH4Cl(s)If 3.0 moles of HCl gas and 3 moles of NH3 gas. each measured at 20oC and 1.0 atmosphere pressure, are allowed to react completely according to the equation above, the final mixture will contain

The correct option is A 3 moles of solid NH4Cl onlyHCl (g)+ NH3 (g) → NH4Cl (s)The chemical reaction is the balanced reaction. Then 3 mole of HCl and ammonia when react they formed 3 moles of ammonium chloride.Ans is A

$H C l (g) + N H_{3} (g) - N H_{4} C l (s)$
If 3.0 moles of HCl gas and 3 moles of $N H_{3}$ gas. each measured at $20^{o} C$ and 1.0 atmosphere pressure, are allowed to react completely according to the equation above, the final mixture will contain

The correct option is A 3 moles of solid $N H_{4} C l$ only
$H C l$ (g)+ $N H_{3}$ (g) $\to$ $N H_{4} C l$ (s)
The chemical reaction is the balanced reaction. Then 3 mole of $H C l$ and ammonia when react they formed 3 moles of ammonium chloride.
Ans is A