Question

The reaction, $2{{\rm{A}}_{\left( {\rm{g}} \right)}} + {{\rm{B}}_{\left( {\rm{g}} \right)}}\leftrightharpoons3{{\rm{C}}_{\left( {\rm{g}} \right)}} + {{\rm{D}}_{\left( {\rm{g}} \right)}}$ is begun with the concentration of $A$ and $B$ both at an initial value of $1.00\;M.$ When equilibrium is reached, the concentration of $D$ is measured and found to be $0.25\;M$. The value for the equilibrium constant for this reaction is given by the expression :

Accepted Answer

$\left[ {{{\left( {0.75} \right)}^3}\left( {0.25} \right)} \right] \div \left[ {{{\left( {0.50} \right)}^2}\left( {0.75} \right)} \right]$

Answer

$\left[ {{{\left( {0.75} \right)}^3}\left( {0.25} \right)} \right] \div \left[ {{{\left( {1.00} \right)}^2}\left( {1.00} \right)} \right]$

Answer

$\left[ {{{\left( {0.75} \right)}^3}\left( {0.25} \right)} \right] \div \left[ {{{\left( {0.50} \right)}^2}\left( {0.25} \right)} \right]$

Answer

$\left[ {{{\left( {0.75} \right)}^3}\left( {0.25} \right)} \right] \div \left[ {{{\left( {0.75} \right)}^2}\left( {0.25} \right)} \right]$

NEET UG CHEMISTRY MCQ: Equilibrium

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