Gaseous hydrogen and gaseous iodine react together to form hydrogen iodide.
H2 + I2 2HI
a The graph shows how the amount of hydrogen iodide varies with time in a 1.00 dm3 container.
The initial amounts of hydrogen and iodine were 1.00 mol H2 and 1.00 mol I2.
Draw a similar graph to show how the number of moles of hydrogen varies with time.
Don't see a graph in the post.
Can't draw a graph on this forum.
To draw a graph showing how the number of moles of hydrogen varies with time in the given reaction, we need to understand the stoichiometry of the reaction and how the reactants are consumed.
The balanced equation for the reaction is:
H2 + I2 → 2HI
According to this equation, for every 1 mole of H2 that reacts, 2 moles of HI are formed. Therefore, the number of moles of hydrogen will decrease by 1 for every 2 moles of HI formed.
We are given that the initial amounts of hydrogen and iodine are both 1.00 mol. Therefore, at the start of the reaction, the number of moles of hydrogen is 1.00 mol.
As the reaction proceeds, the number of moles of hydrogen will decrease. After a certain time, all the hydrogen will be consumed and converted into hydrogen iodide.
To draw the graph, we can assume that the reaction goes to completion and all the hydrogen is consumed. We can consider the number of moles of hydrogen as the y-axis and time as the x-axis.
At time t = 0, the number of moles of hydrogen is 1.00 mol (the initial amount).
As time progresses and the reaction proceeds, for every 2 moles of HI formed, 1 mole of H2 is consumed.
Therefore, at time t = t1 (the time when half the moles of HI are formed), the number of moles of hydrogen will be 1.00 - (1/2) = 0.50 mol.
Similarly, at time t = t2 (the time when all the moles of HI are formed), the number of moles of hydrogen will be 1.00 - (2/2) = 0.00 mol.
So, the graph would start at (0, 1.00) and end at (t2, 0.00), following a straight line decreasing from left to right.
Note: The actual rate at which the reaction occurs might not be a straight line, but we can assume it for simplicity in this case.