If your trading capital is 10 lakh rupees, what is the maximum risk you should take per trade?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:
$CH_4 (g) + H_2O (g) \rightleftharpoons CO (g) + 3H_2 (g)$
(b) How will the values of $K_p$ and composition of equilibrium mixture be affected by
(ii) increasing the temperature

Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(iii) $CO_2 (g) + C (s) \rightleftharpoons 2CO (g)$

Calculate the pH of the following solutions:
d) 1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate $K_{sp} = 7.4 \times 10^{-8}$ ).

Nitric oxide reacts with $Br_2$ and gives nitrosyl bromide as per reaction given below:
$2NO (g) + Br_2 (g) \rightleftharpoons 2NOBr (g)$
When 0.087 mol of NO and 0.0437 mol of $Br_2$ are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and $Br_2$.

A sample of pure $PCl_5$ was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of $PCl_5$ was found to be $0.5 \times 10^{-1}$ mol $L^{-1}$. If value of $K_c$ is $8.3 \times 10^{-3}$, what are the concentrations of $PCl_3$ and $Cl_2$ at equilibrium?
$PCl_5 (g) \rightleftharpoons PCl_3 (g) + Cl_2(g)$

At 473 K, equilibrium constant $K_c$ for decomposition of phosphorus pentachloride, $PCl_5$ is $8.3 \times 10^{-3}$. If decomposition is depicted as,
$PCl_5 (g) \rightleftharpoons PCl_3 (g) + Cl_2 (g)$ $\Delta_r H^{\circ} = 124.0$ kJ $mol^{-1}$
b) what is the value of $K_c$ for the reverse reaction at the same temperature?

Reaction between $N_2$ and $O_2$ takes place as follows:
$2N_2 (g) + O_2 (g) \rightleftharpoons 2N_2O (g)$
If a mixture of 0.482 mol $N_2$ and 0.933 mol of $O_2$ is placed in a 10 L reaction vessel and allowed to form $N_2O$ at a temperature for which $K_c= 2.0 \times 10^{-37}$, determine the composition of equilibrium mixture.

What will be the conjugate bases for the Brönsted acids: HF, $H_2SO_4$ and $HCO_3^{-}$?

Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
(a) Human muscle-fluid, 6.83

The equilibrium constant for the following reaction is $1.6 \times 10^5$ at 1024K
$H_2(g) + Br_2(g) \rightleftharpoons 2HBr(g)$
Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024K.

The ionization constant of chloroacetic acid is $1.35 \times 10^{-3}$. What will be the pH of 0.1M acid and its 0.1M sodium salt solution?

Describe the effect of:
a) addition of $H_2$
on the equilibrium of the reaction:
$2H_2(g) + CO (g) \rightleftharpoons CH_3OH (g)$

At 700 K, equilibrium constant for the reaction:
$H_2 (g) + I_2 (g) \rightleftharpoons 2HI (g)$
is 54.8. If 0.5 mol $L^{-1}$ of $HI(g)$ is present at equilibrium at 700 K, what are the concentration of $H_2(g)$ and $I_2(g)$ assuming that we initially started with $HI(g)$ and allowed it to reach equilibrium at 700K?

Calculate b) the equilibrium constant for the formation of $NO_2$ from NO and $O_2$ at 298K
$NO (g) + \frac{1}{2} O_2 (g) \rightleftharpoons NO_2 (g)$
where
$\Delta_f G^{\circ} (NO_2) = 52.0$ kJ/mol
$\Delta_f G^{\circ} (NO) = 87.0$ kJ/mol
$\Delta_f G^{\circ} (O_2) = 0$ kJ/mol

Calculate the pH of the following solutions:
a) 2 g of TlOH dissolved in water to give 2 litre of solution.

Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(vi) $4 NH_3 (g) + 5O_2 (g) \rightleftharpoons 4NO (g) + 6H_2O(g)$

Predict which of the following reaction will have appreciable concentration of reactants and products:
a) $Cl_2 (g) \rightleftharpoons 2Cl (g) \quad K_c = 5 \times 10^{-39}$

Write the expression for the equilibrium constant, $K_c$ for each of the following reactions:
(i) $2NOCl (g) \rightleftharpoons 2NO (g) + Cl_2 (g)$