For the reaction of H2 with I2, the rate constant is 2.5 × 10–4 dm3 mol–1s–1 at 327°C and 1.0 dm3 mol–1 at 527°C. The activation energy for the reaction, in kJ mole–1 is : (R = 8.314 JK–1 mol–1 )

A bacterial infection in an internal wound grows as N'(t) = N0 exp(t), where the time t is in hours. A does of antibiotic, taken orally, needs 1 hour to reach the wound. Once it reaches there, the bacterial population goes down as {{dN} \over {dt}} = - 5{N^2}. What will be the plot of {{{N_0}} \over N} vs. t after 1 hour?

Consider the given plot of enthalpy of the following reaction between A and B. A+ B $$\to$$ C + D Identify the incorrect statement.

The given plots represent the variation of the concentration of a reactant R with time for two different reactions (i) and (ii). The respective orders of the reactions are :

For a reaction scheme $$A\text{buildrel}{k}_1\frac{⟶}{B}\text{buildrel}{k}_2\frac{⟶}{C}$$, if the rate of formation of B is set to be zero then the concentration of B is given by :

For a reaction consider the plot of $$\ell$$n k versus 1/T given in the figure. If the rate constant of this reaction at 400 K is 10–5 s–1, then the rate constant at 500 K is –

Decomposition of X exhibits a rate constant of 0.05 $$\mu$$g/year. How many year are required for the decomposition of 5$$\mu$$g of X into 2.5 $$\mu$$g?

The reaction 2X $$\to$$ B is a zeroth order reaction. If the initial concentration of X is 0.2 M, the half-life is 6 h. When the initial concentration of X is 0.5 M, the time required to reach its final concentration of 0.2 M will be:

For an elementary chemical reaction, the expression for {{d\left[ A \right]} \over {dt}} is

Consider the given plots for a reaction obeying Arrhenius equation (0oC < T < 300oC) : (K and Ea are rate constant and activation energy, respectively) Choose the correct option :

For the reaction, 2A + B $$\to$$ products, when the concentrations of A and B both were doubled, the rate of the reaction increased from 0.3 mol L$$-$$1s$$-$$1 to 2.4 mol L$$-$$1s$$-$$1. When the concentration of A alone is doubled, the rate increased from 0.3 mol L$$-$$1s$$-$$1 to 0.6 mol L$$-$$1s$$-$$1.

The following results were obtained during kinetic studies of the reaction ; 2A + B $$\to$$ Products .tg {border-collapse:collapse;border-spacing:0;} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg .tg-wv9z{font-size:22px;text-align:center} .tg .tg-de48{font-weight:bold;font-size:22px;text-align:center} Experiment [A] (in mol L$$-$$1) [b] (in mol L$$-$$1) Initial Rate of reaction (In mol L$$-$$1 min$$-$$1) I 0.10 0.20 6.93 G 10$$-$$3 II 0.10 0.25 6.93 G 10$$-$$3 III 0.20 0.30 1.386 G 10$$-$$2 The time (in minutes) required to consume half of A is :

For the reaction 2A + B $$\to$$ C, the values of initial rate at diffrent reactant concentrations are given in the table below. The rate law for the reaction is : .tg {border-collapse:collapse;border-spacing:0;} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg .tg-s6z2{text-align:center} .tg .tg-baqh{text-align:center;vertical-align:top} [A] (mol L-1) [B] (mol L-1) Initial Rate (mol L-1s-1) 0.05 0.05 0.045 0.10 0.05 0.090 0.20 0.10 0.72

Match the catalysts (Column I) with products (Column II). .tg {border-collapse:collapse;border-spacing:0;width:100%} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg .tg-s6z2{text-align:center} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-hgcj{font-weight:bold;text-align:center} Column I Column II (A) V2O5 (i) Polyethylene (B) TiCl4/Al(Me)3 (ii) ethanal (C) PdCl2 (iii) H2SO4 (D) Iron Oxide (iv) NH3

Among the following, the INCORRECT statement about colloids is :

Peptization is a :

The correct option among the following is :

A gas undergoes physical adsorption on a surface and follows the given Freundlich adsorption isotherm equation {x \over m} = k{p^{0.5}} Adsorption of the gas increase with :

The aerosol is a kind of colloid in which :

Adsorption of a gas follows freundlich adosorbed isotherm. x is the mass of the gas adsorbed on mass m of the adsorbent. The plot log x \over m versus log p is shown in the given graph. x \over m is proportional to :