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Fiesta28 [93]
3 years ago
11

Calculate the pressure in atmospheres of 0.5 mol of Helium ( He) at 20°C & occupying 2.50 L.

Chemistry
1 answer:
Morgarella [4.7K]3 years ago
7 0

Answer:

4.811 atm.

Explanation:

  • We can use the general law of ideal gas:<em> PV = nRT.</em>

where, P is the pressure of the gas in atm (P = ?? atm).

V is the volume of the gas in L (V = 2.5 L).

n is the no. of moles of the gas in mol (n = 0.5 mol).

R  is the general gas constant (R = 0.0821 L.atm/mol.K),

T is the temperature of the gas in K (T = 20°C + 273 = 293 K).

<em>∴ P = nRT/V =</em> (0.5 mol)(0.0821 L.atm/mol.K)(293 K)/(2.5 L) = <em>4.811 atm.</em>

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Mn(s)+2HCl(aq)\rightarrow  MnCl_2(aq)+H_2(g)

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m=1.00 g/mL\times 100.0 mL = 100 g

First we have to calculate the heat gained by the solution in coffee-cup calorimeter.

q=m\times c\times (T_{final}-T_{initial})

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T_{initial} = initial temperature = 28.9^oC

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