To find the pressure of the gas at the new conditions, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's convert the initial and final volumes to cubic meters:
Initial volume = 0.50 m^3
Final volume = 0.10 m^3

Next, let's convert the initial and final temperatures to Kelvin:
Initial temperature = 33°C + 273.15 = 306.15 K
Final temperature = -55°C + 273.15 = 218.15 K

Now, let's rearrange the ideal gas law equation to solve for pressure:
P = (nRT) / V

Since the number of moles (n) and the gas constant (R) are constant, we can simplify the equation to:
P1V1 / T1 = P2V2 / T2

Substituting the given values:
P1 = 760 mm Hg
V1 = 0.50 m^3
T1 = 306.15 K
V2 = 0.10 m^3
T2 = 218.15 K

Now we can solve for P2:
P2 = (P1 * V1 * T2) / (V2 * T1)

Plugging in the values:
P2 = (760 mm Hg * 0.50 m^3 * 218.15 K) / (0.10 m^3 * 306.15 K)

Calculating this expression, we find that the pressure of the gas at the new conditions is approximately 1,350 mm Hg.

Question

To find the pressure of the gas at the new conditions, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's convert the initial and final volumes to cubic meters:
Initial volume = 0.50 m^3
Final volume = 0.10 m^3

Next, let's convert the initial and final temperatures to Kelvin:
Initial temperature = 33°C + 273.15 = 306.15 K
Final temperature = -55°C + 273.15 = 218.15 K

Now, let's rearrange the ideal gas law equation to solve for pressure:
P = (nRT) / V

Since the number of moles (n) and the gas constant (R) are constant, we can simplify the equation to:
P1V1 / T1 = P2V2 / T2

Substituting the given values:
P1 = 760 mm Hg
V1 = 0.50 m^3
T1 = 306.15 K
V2 = 0.10 m^3
T2 = 218.15 K

Now we can solve for P2:
P2 = (P1 * V1 * T2) / (V2 * T1)

Plugging in the values:
P2 = (760 mm Hg * 0.50 m^3 * 218.15 K) / (0.10 m^3 * 306.15 K)

Calculating this expression, we find that the pressure of the gas at the new conditions is approximately 1,350 mm Hg.

Knowee AI · Accepted Answer

To find the pressure of the gas at the new conditions, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's convert the initial and final volumes to cubic meters:
Initial volume = 0.50 m^3
Final volume = 0.10 m^3

Next, let's convert the initial and final temperatures to Kelvin:
Initial temperature = 33°C + 273.15 = 306.15 K
Final temperature = -55°C + 273.15 = 218.15 K

Now, let's rearrange the ideal gas law equation to solve for pressure:
P = (nRT) / V

Since the number of moles (n) and the gas constant (R) are constant, we can simplify the equation to:
P1V1 / T1 = P2V2 / T2

Substituting the given values:
P1 = 760 mm Hg
V1 = 0.50 m^3
T1 = 306.15 K
V2 = 0.10 m^3
T2 = 218.15 K

Now we can solve for P2:
P2 = (P1 * V1 * T2) / (V2 * T1)

Plugging in the values:
P2 = (760 mm Hg * 0.50 m^3 * 218.15 K) / (0.10 m^3 * 306.15 K)

Calculating this expression, we find that the pressure of the gas at the new conditions is approximately 1,350 mm Hg.

A compressor takes 0.50 m3 of a gas at 33°C and 760 mm Hg and compresses it to 0.10 m3, cooling it to -55°C at the same time. What is the pressure of the gas at these new conditions?68 mm Hg3.7 x 10 -4 mm Hg2,700 mm Hg1.0 mm Hg

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