Magnesium metal reacts with hydrochlroic acid according to following reaction:
Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2 (g)
over interval of 10.00s, the mass of Mg changes by -0.22g. What is the corresponding rate of consumption of HCl (in Mol/s) ?
So what i think i should do is first convert the rate of consumption to mol/s and then use that to find corresponding rate of consumption of HCl
This is my work
Molar mass of Mg= 24.3
m=-0.22
n=m/M
n=-0.22/24.3 = -0.009 mol
-0.009 is in 10 seconds so
-0.009/10=-0.0009 mol/s
The ratio between Mg and HCl is 1:2
so
2(-0.0009)=-0.0018 Mol/s
So the rate of consumption of HCl is -0.0018 Mol/s
am i doing anything wrong?
Thanks
It looks ok to me. The negative sign is right but I think a consumption of -0.0018 is redundant. I believe the way to state it is a consumption of 0.0018 mol/s.
Oh okay. thanks a lot :)
i don't know the answer
Your calculations are mostly correct, but there is one small error in your final answer. Let's go through the steps to determine the correct rate of consumption of HCl.
Step 1: Convert the mass change of Mg to moles of Mg.
You correctly used the formula n = m/M, where m is the mass change (-0.22 g) and M is the molar mass of Mg (24.3 g/mol). So, n = -0.22 g / 24.3 g/mol = -0.00905 mol.
Step 2: Convert moles of Mg to moles of HCl.
From the balanced chemical equation, we see that the stoichiometric ratio between Mg and HCl is 1:2. Since 1 mole of Mg consumes 2 moles of HCl, the rate of consumption of HCl will be -0.00905 mol/s x 2 = -0.0181 mol/s.
Therefore, the correct rate of consumption of HCl is approximately -0.0181 mol/s. This means that for every second, 0.0181 mol of HCl is being consumed during the reaction.