Answer:
D. The equipment needed to accommodate the high temperature and pressure will be expensive to produce.
Explanation:
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In this case, for the considered reaction, it is clear it is an exothermic reaction because it produces energy; and therefore, the higher the temperature the more reactants are yielded as the reverse reaction is favored. Moreover, since the effect of pressure is verified as favoring the side with fewer moles; in this case the products side (2 moles of ammonia).
In such a way, the high pressure favors the formation of ammonia whereas the high temperature the formation of hydrogen and nitrogen and therefore, option A is ruled out. Since the high pressure shifts the reaction rightwards and the high temperature leftwards, we would not be able to know whether the reaction has ended or not because it will be a "go and come back" process, that is why B is also discarded. Now, since hydrogen and nitrogen would be the "wastes", we discard C because they are not toxic. That is why the most accurate answer would be D. because it is actually true that such equipment is quite expensive.
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2K + Br₂ = 2KBr
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Answer:
13.8%
Explanation:
take the 123g and divide it by the total mass which is 123g + 765g
123/888 = .138
multiply by 100 for a percentage = 13.8%
When heat energy at a constant pressure = the change of enthalpy
ΔH = Q
and when the internal energy of an ideal gas formula is:
ΔH = n.Cp.ΔT
and when Cp = (5/2) R at a constant pressure of a monatomic ideal gas
∴Q = n.(5/2).R.ΔT
∴ ΔT = Q / [n.(5/2).R]
when Q is the heat required = 43.08 J (given)
and n is no.of moles = mass / molar mass
= 1.1 g / 39.948 g/mol
= 0.0275 moles
and R is gas constant = 8.314472J/mol K
by substitution:
ΔT = 43.08 J / (0.0275moles *(5/2) * 8.314472 J/mol K
= 76.76 K
