Answer :

The volume of 4.00 moles of methane gas, CH4, at 19°C and 1.70 atm is approximately 67.6 liters, calculated using the Ideal Gas Law.

To find the volume in liters of 4.00 moles of methane gas, CH4, at 19°C and 1.70 atm, you can use the Ideal Gas Law, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant, and T is the temperature in Kelvin.

First, convert the temperature to Kelvin by adding 273.15 to the Celsius temperature: T = 19 + 273.15 = 292.15 K. Next, use the Ideal Gas Law to solve for volume (V).

Using the values provided:

  • P = 1.70 atm,
  • n = 4.00 moles,
  • R = 0.0821 L·atm/(mol·K) (universal gas constant),
  • T = 292.15 K,

Plugging these into the equation gives us:

V = (nRT)/P = (4.00 moles × 0.0821 L·atm/(mol·K) × 292.15 K) / 1.70 atm

After calculating, the volume V comes out to be approximately 67.6 liters.

The volume of 4.00 moles of methane gas under the given conditions is 67.6 liters.

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Rewritten by : Jeany

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