Madsen chem mastering

P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K). Using the ideal gas law, determine the amount of gas, in moles, of a 8.32 L sample of hydrogen gas, under a temperature of 310 K and a pressure of 1.7 atm.

0.56 mol

A balloon has a volume of 2.55 L, a pressure of 1.15 atm, and a temperature of 25 °C. What is the new pressure, if the new volume is 3.15 L and the new temperature is 45 °C?

0.993 atm

P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K). Consider the following conditions: a sample of neon gas was under 3.0 atm of pressure, a volume of 570 mL with a temperature of 75 °C. Assume you are going to use the ideal gas law to solve for the unknown variable. What variable are you solving for? Are all of variables in the correct units? If not, which variable needs to be converted to the correct units?

1) Moles of gas 2) Volume needs to be converted to L, liters, and temperature needs to be converted to K, Kelvins

P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K). Consider the following conditions: carbon dioxide gas was placed into a 3 L balloon, under a temperature of 305 K, resulting in 2.6 moles of carbon dioxide. Assume you are going to use the ideal gas law to solve for the unknown variable. What variable are you solving for? Are all of variables in the correct units? If not, which variable needs to be converted to the correct units?

1) Pressure 2) All of the variables are in the correct units

P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K). Consider the following conditions: a 3,500 mL tank was filled with 27 moles of argon gas under a pressure of 12 atm. Assume you are going to use the ideal gas law to solve for the unknown variable.What variable are you solving for? Are all of variables in the correct units? If not, which variable needs to be converted to the correct units?

1) Temperature 2) Volume needs to be converted to L, liters

Consider the following conditions: 4.5 moles of helium gas exist under 2.2 atm of pressure and a temperature of 45 °C. Assume you are going to use the ideal gas law to solve for the unknown variable. What variable are you solving for? Are all of variables in the correct units? If not, which variable needs to be converted to the correct units?

1) Volume 2) Temperature needs to be converted to K, Kelvins

A sample of radon gas has a volume of 1.53 L, a pressure of 1.15 atm, and a temperature of 305 K. What is the new pressure, if the new volume is 1.78 and the new temperature is 325 K?

1.05 atm

A sample of sulfur dioxide gas has a volume of 0.871 L and a temperature of 315 K, under a constant pressure. What is the new volume, if the temperature is increased to 385 K?

1.06 L

A sample of helium gas has a volume of 1.25 L and a temperature of 22 °C, under a constant pressure. What is the new volume, if the temperature is increased to 45 °C?

1.35 L

A sample of argon has a volume of 0.983 L, a pressure of 2.50 atm, and a temperature of 32 °C. What is the new volume, if the new pressure is 1.55 atm and the new temperature is 55 °C?

1.71 L

A sample of nitrogen has a volume of 1.75 L, a pressure of 2.00 atm, and a temperature of 35 °C. What is the new temperature, if the new volume is 2.45 L and the new pressure is 1.32 atm?

12 °C

Using the ideal gas law, determine the volume of a 1.43 mole sample of nitrogen gas, under a temperature of 301 K and a pressure of 2.5 atm.

14 L

P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K). Using the ideal gas law, determine the temperature of a 2.63 mole sample of xenon gas, with a volume of 1.60 × 104 mL and under a pressure of 2.20 atm

163 K

A sample of carbon monoxide gas has a volume of 3.45 L and a pressure of 2.82 atm, under a constant temperature of 28 °C. What is the new volume, if the pressure is increased to 4.2 atm?

2.3 L

A sample of water vapor has a volume of 3.15 L, a pressure of 2.40 atm, and a temperature of 325 K. What is the new temperature, if the new pressure is 1.97 atm and the new volume is 2.78 L?

235 K

A sample of chlorine gas has a volume of 2.61 L, a pressure of 0.85 atm, and a temperature of 292 K. What is the new volume, if the new pressure is 0.65 atm and the new temperature is 298 K?

3.5 L

A sample of helium gas has a temperature of 298 K and a pressure of 3.60 atm, under a constant volume. What is the new temperature, if the pressure is increased to 3.80 atm?

315 k

Using the ideal gas law, determine the pressure of a 0.820 mole sample of oxygen gas, under a temperature of 25.0 °C and a volume of 4.78 L.

4.20 atm

A sample of krypton gas has a volume of 5.78 L and a pressure of 2.92 atm, under a constant temperature of 300 K. What is the new volume, if the pressure is decreased to 1.75 atm?

9.64 L

Select the balloon volume that would represent the following conditions: the temperature decreases under constant pressure.

Balloon A, volume decreaseS

Select the balloon volume that would represent the following conditions: the pressure decreases under constant temperature.

Balloon C, volume increases

Select the balloon volume that would represent the following conditions: the temperature is increased by half while the pressure is simultaneously decreased by half.

Balloon C, volume increases

Which statement best describes Gay-Lussac's Law?

Pressure and temperature are directly proportional to one another.

Which statement best describes Boyle's Law?

Pressure and volume are inversely proportional to one another.

What would happen to the pressure of a gas, if the temperature increases, while the volume is held constant?

Pressure increases

Which statement best describes Charles's Law?

Temperature and volume are directly proportional to one another.

A sample of neon gas has a volume of 2.85 L and a temperature of 15 °C, under a constant pressure. What is the new temperature (in °C), if the volume is decreased to 1.45 L?

−126 °C