Answer to Question #109645 in General Chemistry for Joshua

Question

0.72g of my was attached to different volumes of 2mol/dm of HCL the volume of hydrogen liberated was measured at room temperature and pressure the result of the experiment was tabulated below
Volume of HCL used. Vol Of H used
5. 120
15. 360
25. 550
35. .. 600
45. 600
Use the table to plot a graph of the volume of hydrogen liberated against the volume of acid used

Answer 1

The equation that the occurring chemical reaction is : $2M+2HCl (aq)\to 2MCl+H_2(g)$

Thus, every 2 moles of HCl used, liberates 1 mol of Hydrogen gas.

Also, we know that at STP, $1mol= 22.4L$

Thus, every 2 moles of HCl used, liberates 22.4L of Hydrogen gas. ---(a)

Clearly the graph is a straight line, with equation $V_{HCl}=11.2V_{H_2}$ ; ---(from (a))

where ;

$V_{HCl}=$ volume of HCl used in Litres and $V_{H_2}=$ volume of Hydrogen liberated in Litres.

In the graph; Y-axis denotes Volume of HCl used and X-axis denotes the Volume of Hydrogen gas liberated.