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3 years ago

Small children are occasionally injured when they try to inhale helium from

Chemistry

1 answer:

sattari [20]3 years ago

8 0

Answer:

260 moles of Helium

Explanation:

V = 50L

T = 20°C = (20 + 273.15)K = 293.15K

P = 125 atm

R = 0.082 L.atm / mol. K

n = ?

From ideal gas equation,

PV = nRT

P = pressure of a given gas

V = volume it occupies

n = number of moles

R = ideal gas constant

T = temperature of the gas

PV = nRT

n = PV / RT

n = (125 * 50) / (0.082 * 293.15)

n = 6250 / 24.0383

n = 260.00 moles

The child inhaled 260 moles of Helium

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3 years ago

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Answer:

For A: The $K_p$ for the given reaction is $4.0\times 10^1$

For B: The $K_c$ for the given reaction is 1642.

Explanation:

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For A:

The expression of $K_p$ for the above reaction follows:

$K_p=\frac{(p_{NOCl})^2}{(p_{NO})^2\times p_{Cl_2}}$

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$p_{NOCl}=0.24 atm\\p_{NO}=9.10\times 10^{-2}atm=0.0910atm\\p_{Cl_2}=0.174atm$

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For B:

Relation of $K_p$ with $K_c$ is given by the formula:

$K_p=K_c(RT)^{\Delta ng}$

where,

$K_p$ = equilibrium constant in terms of partial pressure = $4.0\times 10^1$

$K_c$ = equilibrium constant in terms of concentration = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature = 500 K

$\Delta ng$ = change in number of moles of gas particles = $n_{products}-n_{reactants}=2-3=-1$

Putting values in above equation, we get:

$4.0\times 10^1=K_c\times (0.0821\times 500)^{-1}\\\\K_c=\frac{4.0\times 10^1}{(0.0821\times 500)^{-1})}=1642$

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