Consider the following chemical reactions performed at identical temperature and volume: Experiment I: X(g) 2 Y(g) Experiment II: X(g) Z(g) The partial pressure of the reactant and product are denoted, respectively, by p_ reactant and p_ product during the course of the reactions. Assuming ideal gas behaviour, the correct plot of p_ reactant versus p_ product for Experiments I and II is:

Step-by-step solution

Let the initial partial pressure of reactant X be P₀ . For Experiment I, X(g) 2Y(g) . If the partial pressure of X decreases by x , then the partial pressure of product Y increases by 2x . We have p_ reactant = P₀ - x and p_ product = 2x , which gives x = p_ product 2 . Substituting this into the first equation, we get p_ reactant = P₀ - 1 2 p_ product . This represents a straight line with a slope of -1/2 and an x-intercept of 2P₀ . For Experiment II, X(g) Z(g) . If the partial pressure of X decreases by y , then