Many gases are produced through chemical reactions inside closed systems in a re

Question

Many gases are produced through chemical reactions inside closed systems in a research lab because only a small amount of the gas is required as a reagent for a further chemical reaction. An example reaction to produce chlorine gas is shown below.

2 HCl (aq) + NaOCl (aq) --> Cl2 (g) + NaCl (aq) + H2O (l)

If 0.2 moles of HCl is reacted with 0.06 moles of NaOCl, what is the change in pressure (?P) assuming that T is 298 K and V is 1.5 Liters? Use 8.314 J/mol K for the ideal gas constant. Record your answer to 3 significant figures.

Explanation / Answer

PV=nRT
P=pressure
V=volume
n= # of moles
R= constant 8.314
T= temp
We right down what we know is constant and leave what isn't as independent variables
P(1.5L)=n1(8.314)(298)
so
P1(1.5)=n2(8.314)(298)
adn
P2(1.5)=n(8.314)(298)
solve for P1 and P2 (divide by the 1.5), and then subtract them,
(Delta)P=n1(8.314)(298)/1.5-n2(8.314)(298)/1.5
n1 is just .2mols (The original amount)
n2 is just .26 (The original + reactant)
And you should get... -99.102

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