320171 Assertion :
In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason :
It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

320172 The rate of gaseous reaction is given by the expression \({\rm{k[A][B}}{{\rm{]}}^{\rm{2}}}\). If the volume of vessel is reduced to one half of the initial volume, the reaction rate as compared to to original rate is

320173 For the gaseous reaction \({\rm{2A + B}} \to {\rm{C + D}}\) the differential rate law is \(\frac{{{\rm{dx}}}}{{{\rm{dt}}}}{\rm{ = k[A]}} \cdot {\rm{[B]}}\). The volume of the container containing the reaction mixture is reduced to\(\frac{{{{\rm{1}}^{{\rm{th }}}}}}{{\rm{4}}}\) of the original volume. The rate of reaction will change by

320174 Assertion :
The rate law equation can be found only by experiment.
Reason :
It can be written from stoichiometric equation.

320175 Assertion :
The kinetics of the reaction, \({\text{mA + nB + pC}} \to {m^\prime }X + {n^\prime }Y + {p^\prime }Z\) obeys the rate expression as \(\dfrac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}[\mathrm{A}]^{\mathrm{m}}[\mathrm{B}]^{\mathrm{n}}\)
Reason :
The rate of reaction does not depend upon the concentration of \(\mathrm{C}\).

320171 Assertion :
In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason :
It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

320172 The rate of gaseous reaction is given by the expression \({\rm{k[A][B}}{{\rm{]}}^{\rm{2}}}\). If the volume of vessel is reduced to one half of the initial volume, the reaction rate as compared to to original rate is

320173 For the gaseous reaction \({\rm{2A + B}} \to {\rm{C + D}}\) the differential rate law is \(\frac{{{\rm{dx}}}}{{{\rm{dt}}}}{\rm{ = k[A]}} \cdot {\rm{[B]}}\). The volume of the container containing the reaction mixture is reduced to\(\frac{{{{\rm{1}}^{{\rm{th }}}}}}{{\rm{4}}}\) of the original volume. The rate of reaction will change by

320174 Assertion :
The rate law equation can be found only by experiment.
Reason :
It can be written from stoichiometric equation.

320175 Assertion :
The kinetics of the reaction, \({\text{mA + nB + pC}} \to {m^\prime }X + {n^\prime }Y + {p^\prime }Z\) obeys the rate expression as \(\dfrac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}[\mathrm{A}]^{\mathrm{m}}[\mathrm{B}]^{\mathrm{n}}\)
Reason :
The rate of reaction does not depend upon the concentration of \(\mathrm{C}\).

320171 Assertion :
In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason :
It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

320172 The rate of gaseous reaction is given by the expression \({\rm{k[A][B}}{{\rm{]}}^{\rm{2}}}\). If the volume of vessel is reduced to one half of the initial volume, the reaction rate as compared to to original rate is

320173 For the gaseous reaction \({\rm{2A + B}} \to {\rm{C + D}}\) the differential rate law is \(\frac{{{\rm{dx}}}}{{{\rm{dt}}}}{\rm{ = k[A]}} \cdot {\rm{[B]}}\). The volume of the container containing the reaction mixture is reduced to\(\frac{{{{\rm{1}}^{{\rm{th }}}}}}{{\rm{4}}}\) of the original volume. The rate of reaction will change by

320174 Assertion :
The rate law equation can be found only by experiment.
Reason :
It can be written from stoichiometric equation.

320175 Assertion :
The kinetics of the reaction, \({\text{mA + nB + pC}} \to {m^\prime }X + {n^\prime }Y + {p^\prime }Z\) obeys the rate expression as \(\dfrac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}[\mathrm{A}]^{\mathrm{m}}[\mathrm{B}]^{\mathrm{n}}\)
Reason :
The rate of reaction does not depend upon the concentration of \(\mathrm{C}\).

320171 Assertion :
In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason :
It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

320172 The rate of gaseous reaction is given by the expression \({\rm{k[A][B}}{{\rm{]}}^{\rm{2}}}\). If the volume of vessel is reduced to one half of the initial volume, the reaction rate as compared to to original rate is

320173 For the gaseous reaction \({\rm{2A + B}} \to {\rm{C + D}}\) the differential rate law is \(\frac{{{\rm{dx}}}}{{{\rm{dt}}}}{\rm{ = k[A]}} \cdot {\rm{[B]}}\). The volume of the container containing the reaction mixture is reduced to\(\frac{{{{\rm{1}}^{{\rm{th }}}}}}{{\rm{4}}}\) of the original volume. The rate of reaction will change by

320174 Assertion :
The rate law equation can be found only by experiment.
Reason :
It can be written from stoichiometric equation.

320175 Assertion :
The kinetics of the reaction, \({\text{mA + nB + pC}} \to {m^\prime }X + {n^\prime }Y + {p^\prime }Z\) obeys the rate expression as \(\dfrac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}[\mathrm{A}]^{\mathrm{m}}[\mathrm{B}]^{\mathrm{n}}\)
Reason :
The rate of reaction does not depend upon the concentration of \(\mathrm{C}\).

320171 Assertion :
In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason :
It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

320172 The rate of gaseous reaction is given by the expression \({\rm{k[A][B}}{{\rm{]}}^{\rm{2}}}\). If the volume of vessel is reduced to one half of the initial volume, the reaction rate as compared to to original rate is

320173 For the gaseous reaction \({\rm{2A + B}} \to {\rm{C + D}}\) the differential rate law is \(\frac{{{\rm{dx}}}}{{{\rm{dt}}}}{\rm{ = k[A]}} \cdot {\rm{[B]}}\). The volume of the container containing the reaction mixture is reduced to\(\frac{{{{\rm{1}}^{{\rm{th }}}}}}{{\rm{4}}}\) of the original volume. The rate of reaction will change by

320174 Assertion :
The rate law equation can be found only by experiment.
Reason :
It can be written from stoichiometric equation.

320175 Assertion :
The kinetics of the reaction, \({\text{mA + nB + pC}} \to {m^\prime }X + {n^\prime }Y + {p^\prime }Z\) obeys the rate expression as \(\dfrac{\mathrm{dx}}{\mathrm{dt}}=\mathrm{k}[\mathrm{A}]^{\mathrm{m}}[\mathrm{B}]^{\mathrm{n}}\)
Reason :
The rate of reaction does not depend upon the concentration of \(\mathrm{C}\).