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Answer :
Final answer:
The pressure of the gas can be calculated using the ideal gas law PV=nRT. By plugging the values given in the question into this formula, we determine that the pressure is approximately 2.032 atmospheres.
Explanation:
This question involves using the ideal gas law, which is represented as PV=nRT. In this equation, P represents pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in kelvins.
Here, the volume of the gas (V) is given as 95.2 liters, the amount of gas (n) is given as 7.5 moles, and the temperature (T) is given as 313K. We want to calculate the pressure (P). The value for the ideal gas constant (R) will be 0.0821 L·atm/mol·K when the volume is in liters and the pressure is in atmospheres.
Plugging these values into the formula gives us: P = nRT/V = (7.5 mol * 0.0821 L·atm/mol·K * 313 K) / 95.2 L.
Performing these calculations results in a pressure of approximately 2.032 atmospheres.
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Final answer:
The gas's pressure can be calculated using the PV=nRT equation, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. The gas constant, R, is chosen based on the units used. Plugging in the given values and solving for P will give the required pressure.
Explanation:
The pressure of a gas can be calculated using the Ideal Gas Law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant and T is temperature in Kelvin. Given the number of moles (n=7.5) and temperature (T=313K), but using volume as liters instead of the standard cubic meters, the ideal gas constant (R) appropriate for this situation is 0.08206 L atm mol⁻¹ K⁻¹. By rearranging the equation, we get P = nRT/V, so the pressure would be P = (7.5 mol) * (0.08206 L atm mol⁻¹ K⁻¹)*(313K) / 95.2L. Calculating this expression will give the required pressure in atm.
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