Ammonium carbamate (NH_2COONH_4) when heated | vedclass

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(D) The dissociation reaction is: $NH_2COONH_4(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$.Here,the number of moles of gaseous products $n = 2 + 1 = 3$.

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$1$

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(D) The dissociation reaction is: $NH_2COONH_4(s) ightleftharpoons 2NH_3(g) + CO_2(g)$.Here,the number of moles of gaseous products $n = 2 + 1 = 3$.The molar mass of ammonium carbamate is $M = 78 \, g/mol$.The theoretical vapour density $D_t = \frac{M}{2} = \frac{78}{2} = 39$.The observed vapour density $D_o = 13.0$.The degree of dissociation $\alpha$ is given by the formula: $\alpha = \frac{D_t - D_o}{D_o(n - 1)}$.Substituting the values: $\alpha = \frac{39 - 13}{13(3 - 1)} = \frac{26}{13 	imes 2} = \frac{26}{26} = 1$.

Ammonium carbamate $(NH_2COONH_4)$ when heated to $200\,^{\circ}C$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $13.0$ at equilibrium. What is the degree of dissociation of ammonium carbamate?

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