Q2 of 10 Page 68


a) Identify the reactants and products.


b) Products are frequently removed from the system. Explain the reason.

a) Reactants = C(s) and H2O(g)

Products = CO(g) and H2(g)


The substances which reacts are called reactants and the substances which formed during reaction are called products.


b) We know that According to Le Chatelier principle if we change the concentration of a system at equilibrium then the system will try to cancel the effect of that change and it will attain a new state of equilibrium. So when we remove the products then product molecules will decrease so the reaction will proceed in a forward direction to attain the equilibrium. And so the products will increase.


Note- Equilibrium is that state when the rate of forward reaction becomes equal to the rate of backward reaction.


More from this chapter

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1

a) In which of the following reversible reactions does the change in pressure not influence equilibrium? What is the reason?

i) H2(g) + I2 (g)⇋ 2HI(g)


ii) N2(g) + 3H2(g) ⇋ 2NH3(g)


b) What is the use of applying high pressure during formation of ammonia from nitrogen and hydrogen?

3


a) Which gas is brown in colour?


b) How does an increase in temperature influence the state of equilibrium?


c) How can the yield of the product NO2 be increased?

 4

The chemical equation for the reaction between marble and dilute HCl is given.

CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + CO2 (g) + H2O (l)


a) Which is the gas formed here?


b) Suggest two methods for increasing the rate of reaction. Explain the reason for your suggestions.

 5

2NO(g) + O2(g) ⇋ 2NO2(g) + heat

In this reaction how do the following changes influence the amount of the product?


a) Decrease in temperature


b) Increase in pressure


c) Increase in the concentration of oxygen