An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7g of water freezes at 272.813 K. If the value of K_f for water is 1.86 K/m, what is the molecular mass of the monobasic acid?

Q. Calculate the change in pressure (in atm), when 2 moles of NO and 16 g

O_{2}

in a 6.25 litre originally at

27^{\circ} C

react to produce the maximum quantity of

N O_{2}

possible according to the equation.

2 N O (g) + O_{2} (g) \to 2 N O_{2} (g)

[T a k e R = \frac{1}{12} L a t m K^{1} m o l^{- 1}]

Q. Two equations are simultaneously existing in a vessel at

25^{o} C

N O (g) + N O_{2} (g) ⇌ N_{2} O_{3} (g); K_{P 1}

(say)
If initially only

N O

and

N O_{2}

are present in a

3 : 5

mole ration and the total pressure at equilibrium is 5.5 atm with the pressure of

N O_{2}

0.5 a t m,

calculate

K_{P 1}

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2NO(g)+O2(g)⇌2NO2(g)+150 kJIf 60 g of NO and 60 g of O2 are available, what is the maximum amount of NO2 that can be produced? (Molecular weights: NO=30 g/mole, NO2=46 g/mole)

$2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g) + 150$ kJ
If $60$ g of $N O$ and $60$ g of $O_{2}$ are available, what is the maximum amount of ${N O}_{2}$ that can be produced?
(Molecular weights: $N O = 30$ g/mole, ${N O}_{2} = 46$ g/mole)