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Answer :
Using the Ideal Gas Law, PV=nRT, and rearranging it to V=nRT/P, the volume of 4.00 moles of methane gas at 19°C and 1.70 atm is calculated to be approximately 71.06 liters.
The volume of 4.00 moles of methane gas (CH4) at 19°C (which is 292K when converted from Celsius to Kelvin) and 1.70 atm can be calculated using the Ideal Gas Law, which is expressed as PV=nRT. To solve for V (volume), rearrange the equation to V=nRT/P.
In this case:
- n = 4.00 moles
- R = 0.0821 L ext{atm}/ ext{mol} ext{K} (the ideal gas constant)
- T = 292 K (19°C + 273.15)
- P = 1.70 atm
Plugging these values into the equation gives:
V = (4.00 moles) ext{*} (0.0821 L ext{atm}/ ext{mol} ext{K}) ext{*} (292 K) / (1.70 atm)
After calculating, the volume V is approximately 71.06 liters.
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