Δ H reaction = q / n where q: amount of heat released and n is number of moles of substance.
q = m . C . ΔT where:
m = mass of substance (g)
C = Specific heat capacity (4.18)
ΔT = change in temperature = 24.25 - 23.16 = 1.09
q = 1000 x 4.18 x 1.09 = 4556 J = 4.556 kJ
number of moles (n) = Molarity (M) x Volume (L)
= 0.185 M x 0.07 L = 0.01295 mole
Δ H = q / n = - (4.556 kJ / 0.01295 mole) = -351.8 kJ / mol
Note: it is exothermic reaction (-ve sign) i.e. temperature is raised
Answer:
There are two possible answers to the question
I) decreasing the pressure of the system
II) decreasing the temperature of the system
Explanation:
Looking at the equation of the reaction, it can be seen that the reaction is endothermic. This implies that decreasing the temperature favours the reverse reaction and more NO2 is produced.
Secondly, decreasing the pressure drives the equilibrium position towards the side having the higher total volume hence decreasing the pressure favours the reverse reaction and more NO2 is produced.
Answer:
You know, i always say no but when i watch one i get addicted so... yeah. thanks for the positive messages
Explanation:
When the chemicals combine, it creates a chemical reaction or "eruption"
Answer:
6.054×10²⁵
Explanation:
1)find number of moles of zinc
2)multiply the mole of zinc with 2
3)use the formula mol = number of particle/ avogadro constant
