Question

Assume that an ideal gas of NH_{3} is placed in an
isolated container of 1,600 cm^{3} at 298 K. When the
container is heated to 500 K, NH_{3} is partially
decomposed to N_{2} and H_{2}. The pressure is
found to be 4.50 MPa. Find the number of moles of NH_{3},
N_{2} and H_{2}.

Answer #1

**Either we have to specify the initial pressure or we
have to consider that initial 1 mole of NH3.**

**There after pressure will depends on the mole and
temperature since volume is constant throughout the
pressure.**

#5.133
A mixture of NH3(g) and N2H4(g) is placed in a
sealed container at 320 K . The total pressure is 0.53 bar . The
container is heated to 1200 K at which time both substances
decompose completely according to the equations
2NH3(g)→N2(g)+3H2(g) ;
N2H4(g)→N2(g)+2H2(g) . After
decomposition is complete the total pressure at 1200 K is found to
be 4.5 bar.
Find the percent (by volume) of N2H4(g) in the original
mixture. (Assume two significant figures for the temperature.)

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b. pressure quadruple
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a
b
c
d
e
incorrect
IncorrectQuestion 2
0 / 1 pts
There are 3 balloons sitting next to each other, each of a
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. A container has n = 3 moles of a monoatomic ideal gas at a
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