Question 1

A particular gas exerts a pressure of 4.33 bar.What is this pressure in units of atmospheres?

Accepted Answer

D

Question 2

A flexible vessel contains 43 L of gas where the pressure is 1.3 atm.What will the volume be when the pressure is 0.61 atm,the temperature remaining constant?

Accepted Answer

Using Boyle's Law (P1V1 = P2V2), where P1 = 1.3 atm, V1 = 43 L, and P2 = 0.61 atm, we solve for V2: V2 = (P1V1)/P2 = (1.3 * 43) / 0.61 ≈ 92 L.

Question 3

A particular gas exerts a pressure of 2.52 bar.What is this pressure in units of pascals?

Accepted Answer

One bar is equal to 100,000 Pascals. Therefore, 2.52 bar is equal to 2.52 x 100,000 = 252,000 Pascals.
Written in scientific notation, this is 2.52 x 10^5 Pascals. The correct answer is option C, which is written in scientific notation as 2.52 x 10^5 Pa.

Question 4

A 2.00-L glass soda bottle filled only with air is tightly capped at 25°C and 728.0 mmHg.If the bottle is placed in water at 65°C,what is the pressure in the bottle?

Accepted Answer

The pressure in the bottle can be calculated using the ideal gas law and the fact that the volume and the amount of gas remain constant. The formula to use is $ P_1/T_1 = P_2/T_2 $, where $ P_1 $ and $ T_1 $ are the initial pressure and temperature, and $ P_2 $ and $ T_2 $ are the final pressure and temperature. Temperatures must be in Kelvin. Converting temperatures to Kelvin: $ T_1 = 25°C + 273.15 = 298.15 K $ and $ T_2 = 65°C + 273.15 = 338.15 K $. Solving for $ P_2 $, $ P_2 = P_1 \times (T_2/T_1) = 728.0 \, mmHg \times (338.15 K / 298.15 K) = 826 \, mmHg $.

Question 5

A flexible vessel contains 78.00 L of gas at a pressure of 1.50 atm.Under conditions of constant temperature and moles of gas,what is the pressure of the gas when the volume of the vessel is tripled?

Accepted Answer

According to Boyle's Law, PV = constant at constant temperature and moles of gas. Therefore, P1V1 = P2V2.
Given: P1 = 1.5 atm, V1 = 78.00 L, V2 = 3*V1 = 234 L
Therefore, P2 = P1V1/V2 = (1.5 atm * 78.00 L) / 234 L = 0.5 atm = 0.572 atm (rounded to three significant figures). 
Therefore, the best choice is A, which matches this calculation.

Question 6

Absolute zero is the point at which

Accepted Answer

Absolute zero is defined as the temperature at which the volume of an ideal gas would theoretically reach zero. Therefore, the best choice is the graph of V versus T (K), where the intersection with the origin represents zero volume at zero Kelvin.

Question 7

A particular gas exerts a pressure of 4.09 × 10⁴ Pa.What is this pressure in units of atmospheres?

Accepted Answer

The answer of A particular gas exerts a pressure of...

Question 8

A flexible vessel is filled to a certain pressure with 28.00 L of gas.Under conditions of constant temperature and moles of gas,how does the pressure of the gas change when the volume of the gas is tripled?

Accepted Answer

According to Boyle's Law, at constant temperature and moles of gas, pressure and volume are inversely proportional. Therefore, if the volume is tripled, the pressure must decrease by a factor of three to maintain the same amount of gas at constant temperature.

Question 9

The pressure of a certain gas is measured to be 264.6 mmHg.What is this pressure expressed in units of pascals?​

Accepted Answer

To convert mmHg to pascals, use the conversion factor: 1 mmHg = 133.322 Pa. Therefore, 264.6 mmHg × 133.322 Pa/mmHg = 35279.5 Pa, which is approximately 3.528 × 10⁴ Pa.

Question 10

It is possible to make a barometer using a liquid other than mercury.What would be the height (in meters)of a column of dichloromethane at a pressure of 0.830 atm,given that 0.830 atm is equal to a 0.63522 m column of mercury and the densities of mercury and dichloromethane are 13.5 g/cm³ and 1.33 g/cm³,respectively.

Accepted Answer

The height of the dichloromethane column can be calculated using the principle that the pressure exerted by a column of fluid is given by $P = \rho gh$, where $P$ is the pressure, $\rho$ is the density of the fluid, $g$ is the acceleration due to gravity, and $h$ is the height of the fluid column. Given that the pressure is the same for both mercury and dichloromethane, we can set up a ratio of the heights based on the inverse ratio of their densities, since $h \propto \frac{1}{\rho}$. Given the height of the mercury column is 0.63522 m and its density is 13.5 g/cm³, and the density of dichloromethane is 1.33 g/cm³, the height of the dichloromethane column can be calculated as follows:$$h_{\text{DCM}} = h_{\text{Hg}} \times \frac{\rho_{\text{Hg}}}{\rho_{\text{DCM}}} = 0.63522 \times \frac{13.5}{1.33} \approx 6.4641 \, \text{m}$$This calculation shows that the height of the dichloromethane column under the same pressure would be significantly taller than that of mercury due to its much lower density.

Question 11

A particular gas exerts a pressure of 689 mmHg.What is this pressure in units of bar?

Accepted Answer

The answer of A particular gas exerts a pressure of...

Question 12

A particular gas exerts a pressure of 4.02 atm.What is this pressure in units of bar?

Accepted Answer

To convert atm to bar, we use the conversion factor 1 atm = 1.01325 bar
So, 4.02 atm = 4.02 x 1.01325 bar = 4.07 bar (rounded to two decimal places) 
Therefore, the correct answer is C.

Question 13

A particular gas exerts a pressure of 731 mmHg.What is this pressure in units of atmospheres?

Accepted Answer

The answer of A particular gas exerts a pressure of...

Question 14

The following volume-temperature plots were made at different values of constant pressure while the number of moles of gas in each experiment remained the same.Which plot represents measurements at the highest pressure?

Accepted Answer

The answer of The following volume-temperature plots were made at...

Question 15

A sample of methane,CH₄,occupies a volume of 318.0 mL at 25°C and exerts a pressure of 1010.0 mmHg.If the volume of the gas is allowed to expand to 770.0 mL at 298 K,what will be the pressure of the gas?

Accepted Answer

First, we need to use the ideal gas law formula to find the initial number of moles of methane:

PV = nRT

n = PV/RT

n = (1010.0 mmHg)(318.0 mL)/(62.36 L mmHg K^-1 mol^-1)(298 K)

n = 0.0400 mol

Now, we can use the same formula with the new volume and the same number of moles to find the new pressure:

PV = nRT

P = nRT/V

P = (0.0400 mol)(62.36 L mmHg K^-1 mol^-1)(298 K)/(770.0 mL)

P = 417.1 mmHg

Therefore, the answer is C) 417.1 mmHg.

Question 16

The pressure of a certain gas is measured to be 4.304 × 10³ Pa.What is this pressure expressed in units of mmHg?

Accepted Answer

To convert pressure from pascals (Pa) to millimeters of mercury (mmHg), you can use the conversion factor 1 Pa = 0.00750062 mmHg. Given the pressure is 4.304 × 10^3 Pa, multiplying by the conversion factor gives approximately 32.28 mmHg.

Question 17

A particular gas exerts a pressure of 5.56 × 10⁴ Pa.What is this pressure in units of bar?

Accepted Answer

1 bar is equivalent to 100,000 Pa (1 × 10^5 Pa). Therefore, to convert 5.56 × 10^4 Pa to bar, you divide by 100,000 (1 × 10^5), which gives 0.556 bar.

Question 18

A particular gas exerts a pressure of 2.42 atm.What is this pressure in units of mmHg?

Accepted Answer

The answer of A particular gas exerts a pressure of...

Question 19

When the valve between the 2.00-L bulb,in which the gas pressure is 2.50 atm,and the 3.00-L bulb,in which the gas pressure is 1.50 atm,is opened,what will be the final pressure in the two bulbs? Assume the temperature remains constant.

Accepted Answer

The answer of When the valve between the 2.00-L bulb,in...

Question 20

A flexible vessel contains 37 L of gas where the pressure is 1.0 atm.What will the volume be when the pressure is 0.70 atm,the temperature remaining constant?

Accepted Answer

Using Boyle's Law (P1V1 = P2V2), where P1 = 1.0 atm, V1 = 37 L, and P2 = 0.70 atm, we solve for V2: V2 = (P1V1)/P2 = (1.0 atm * 37 L) / 0.70 atm = 52.86 L, which rounds to 53 L.

Quiz 5: The Gaseous State

A particular gas exerts a pressure of 4.33 bar.What is this pressure in units of atmospheres?

A flexible vessel contains 43 L of gas where the pressure is 1.3 atm.What will the volume be when the pressure is 0.61 atm,the temperature remaining constant?

A particular gas exerts a pressure of 2.52 bar.What is this pressure in units of pascals?

A 2.00-L glass soda bottle filled only with air is tightly capped at 25°C and 728.0 mmHg.If the bottle is placed in water at 65°C,what is the pressure in the bottle?

A flexible vessel contains 78.00 L of gas at a pressure of 1.50 atm.Under conditions of constant temperature and moles of gas,what is the pressure of the gas when the volume of the vessel is tripled?

Absolute zero is the point at which

A particular gas exerts a pressure of 4.09 × 104 Pa.What is this pressure in units of atmospheres?​

A flexible vessel is filled to a certain pressure with 28.00 L of gas.Under conditions of constant temperature and moles of gas,how does the pressure of the gas change when the volume of the gas is tripled?

The pressure of a certain gas is measured to be 264.6 mmHg.What is this pressure expressed in units of pascals?​

A particular gas exerts a pressure of 689 mmHg.What is this pressure in units of bar?

A particular gas exerts a pressure of 4.02 atm.What is this pressure in units of bar?

A particular gas exerts a pressure of 731 mmHg.What is this pressure in units of atmospheres?

The following volume-temperature plots were made at different values of constant pressure while the number of moles of gas in each experiment remained the same.Which plot represents measurements at the highest pressure?

A sample of methane,CH4,occupies a volume of 318.0 mL at 25°C and exerts a pressure of 1010.0 mmHg.If the volume of the gas is allowed to expand to 770.0 mL at 298 K,what will be the pressure of the gas?

The pressure of a certain gas is measured to be 4.304 × 103 Pa.What is this pressure expressed in units of mmHg?​

A particular gas exerts a pressure of 5.56 × 104 Pa.What is this pressure in units of bar?

A particular gas exerts a pressure of 2.42 atm.What is this pressure in units of mmHg?

When the valve between the 2.00-L bulb,in which the gas pressure is 2.50 atm,and the 3.00-L bulb,in which the gas pressure is 1.50 atm,is opened,what will be the final pressure in the two bulbs? Assume the temperature remains constant.

A flexible vessel contains 37 L of gas where the pressure is 1.0 atm.What will the volume be when the pressure is 0.70 atm,the temperature remaining constant?

A particular gas exerts a pressure of 4.09 × 10⁴ Pa.What is this pressure in units of atmospheres?

The pressure of a certain gas is measured to be 264.6 mmHg.What is this pressure expressed in units of pascals?

A sample of methane,CH₄,occupies a volume of 318.0 mL at 25°C and exerts a pressure of 1010.0 mmHg.If the volume of the gas is allowed to expand to 770.0 mL at 298 K,what will be the pressure of the gas?

The pressure of a certain gas is measured to be 4.304 × 10³ Pa.What is this pressure expressed in units of mmHg?

A particular gas exerts a pressure of 5.56 × 10⁴ Pa.What is this pressure in units of bar?