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storchak [24]
3 years ago
11

The pressure of 1 mol of gas is decreased to 0.5 atm at 273 K. What happens to the molar volume of the gas under these condition

s?
Chemistry
1 answer:
m_a_m_a [10]3 years ago
6 0

Answer : The molar volume of the gas will be, 44.82 L

Solution :

Using ideal gas equation,

PV=nRT

where,

n = number of moles of gas  = 1 mole

P = pressure of the gas = 0.5 atm

T = temperature of the gas = 273 K

R = gas constant = 0.0821 Latm/moleK

V = volume of the gas.

Now put all the given values in the above equation, we get the molar volume of the gas.

(0.5atm)\times V=(1mole)\times (0.0821Latm/moleK)\times (273K)

V=44.82L

Therefore, the molar volume of the gas will be, 44.82 L

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<h3>Explanation:</h3>
  • To calculate the amount of heat absorbed or released by a substance we need to know its mass, change in temperature and its specific heat capacity.
  • Then to get quantity of heat absorbed or lost we multiply mass by specific heat capacity and change in temperature.
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in our question we are given;

Mass of copper, m as 95.4 g

Initial temperature = 25 °C

Final temperature = 48 °C

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We are required to calculate the specific heat capacity of copper

Rearranging the formula we get

c = Q ÷ mΔT

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Specific heat capacity, c = 849 J ÷ (95.4 g × 23°C)

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