The equivalence point is the point in a titration where the amount of titrant added is enough to completely neutralize the analyte solution. The moles of titrant (standard solution) equal the moles of the solution with unknown concentration. ... The equivalence point is not the same as the endpoint of a titration.
Using charles law
v1/t1=v2/t2
v1=49ml
v2=74
t1=7+273=280k
t2=?
49/280=74/t2
0.175=74/t2 cross multiply
0.175t2=74
t2=74/0.175
t2=422k or 149celcius
0.2346g of C8H18/114.224g x 6.022 x 10^20 mol of C8H18 =
0.01237 or 1.237x10^20 mol of C8H18.
The amount of oxygen needed would be 80.19 grams
<h3>Stoichiometric problems</h3>
From the equation of the reaction:
The mole ratio of oxygen and ammonia is 3:4
Mole of 56.8g ammonia = 56.8/17 = 3.34 moles
Equivalent mole of oxygen = 3/4 x 3.34 = 2.5059 moles
Mass of 2.5059 moles oxygen = 2.5059 x 32 = 80.19 grams
More on stoichiometric problems can be found here: brainly.com/question/15047541
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