Fe + 2 HCl --> FeCl2 + H2 <span>
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
<span>total moles H2 = 0.100 g / (2.016 g/mol) =0.0496 mol
let x = mass Fe
let y = mass Al
</span></span>
<span>Total mass of alloy is:
<span>x + y = 2.07
</span></span>
<span>Performing H2 balance based on stoichiometry:
<span>x / 55.847 + 3 y/2 / 26.9815 = 0.0496
x / 55.847 + 3y/53.963 = 0.0496
<span>53.963 x + 167.541 y = 149.48
<span>53.967 ( 2.07 - y) + 167.541 y = 149.48
<span>111.71 - 53.967 y + 167.541 y = 149.48
<span>113.6 y = 37.77
y = 0.332 g = mass Al
% Al = 0.332 x 100/ 2.07 = 16.06 %
<span>% Fe = 83.94%</span></span></span></span></span></span></span>
I think you want to ask about Keq. At equilibrium, we can know [SO2Cl2] is 2.2*10-2 M -1.3*10-2M=9*10^-3 M. And [SO2]=[Cl2]. So the Keq=1.88*10^-2.
Endothermic is when the compound absorbs energy in the reaction. Exothermic is the opposite: the compound releases energy in the reaction.
Answer: I think it’s A sorry if I’m wrong
Explanation:
Answer:
40 g aluminum
Explanation:
More residual heat will build up in the increased amount of aluminum atoms