An ideal gas is one which obeys the equation pV / T = constant
(b)
(i)
pV = nRT
{Temperature in Kelvin = 273 + XX = 296 K}
X.0 × XX7× 3.0 × XX–X= n × 8.31 × XXX
XXXXXX of moles, n = X.1 XXX
(ii)
{pV = XXX. XXX XXXXXXXX p is proportional to the XXXXXX XX XXXXXXXXX, n}
Pressure∝Amount of substance
{XXX XXXXX pressure is XXX% - 0.XX% = XX.X% of XXX original pressure. XXXX is, X.XX% has XXXX XXXX. XX, the amount XX XXXXXXXXX XXXX is also X.40% XX XXX XXXXXXXX amount XXXXX XXX XXXXXXXX is XXXXXXXXXXXX to the XXXXXX XX substance. The original XXXXXX XX substance (100%) is X.X mol, XX calculated XXXXX.}
Loss = 0.XX / XXX × 6.X mol = X.0244 mol
{Since XXX XXXXXXX XXXX XX XXXXX in ‘atoms XXX second’, we need XX XXXXXXX XXX amount XX moles into number of XXXXX.}
XXXX = 0.XXXX × 6.02 × XX23(XXXXX) = 1.47 × 10XXatoms
{XXX, XXXX XXXXXX XX XXXXX has XXXX lost in 35 XXXX. To find the XXXX, XX XXXX XX XXXXXXXXX XXX amount XX atoms XXXX in XXX second.}
Rate = (1.XX × 1022) / (XX × XX × 60 × XX) = 4.X × XXXXs–1
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