A 25.0mL expandable container of nitrogen was placed in a pressurized furnace at 4.0atm. The temperature rose from 25°C to 40°C. Assuming constant pressure, what is the volume (mL) of the gas after heating?

0.52 mol of argon gas is admitted to an evacuated 3.00 liter (3.00 × 10-3 m3) container at 20.0°C. What is the pressure of the gas, in atm? 1.00 atm = 1.00×105 Pa.

A 0.0500-g sample of magnesium is reacted with 25 mL of 3.0 M sulfuric acid as described in the experimental section. The resulting hydrogen gas is collected over water and is found to have a volume of 51.0 ml. Thetemperature is 25 °C and the atmospheric pressure is 760.00 mm Hg. The column of water height inside thegraduated cylinder is found to be 24.0 mm. 4.What is the number of moles of hydrogen gas in the sample?5. What is the number of moles of metal in the sample? 6. What is the calculated molar mass of the metal for this trial? 7. What is the percent error in this determination?

A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.07 L1.07 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 15.0 atm,15.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

2.00L of carbon dioxide gas (the main component of the Martian atmosphere) is contained at a pressure of 101.3 kPa at room temperature (21oC) on Earth. The daytime temperature at the equator during summer on Mars is also 21oC. If the atmospheric pressure on Mars is 6.01 mmHg, what volume would the gas occupy on Mars?

The density of a gas is 1.43 g/Lg/L at a temperature of 23 ∘C∘C and a pressure of 0.789 atmatm. Calculate the molar mass of the gas.

Magnesium  metal reacts with molecular  chlorine  gas to form  magnesium   chloride . A closed container of volume  3 .00 x 103 mL contains  chlorine  gas at  2.26  °C and  6.52  x 105 Pa. Then  7.68  g of solid magnesium  is introduced, and the reaction goes to completion. What is the final pressure (in bar) if the temperature rises to  95.06  °C?

A sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.

For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of −196. °C. Suppose the temperature of a sample of nitrogen gas is lowered from 99.0 °C to 80.0 °C, and at the same time the pressure is increased by 5.0%. Does the volume of the sample increase, decrease, or stay the same? If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. increase decrease stays the same % x10 X Ś ? ollo 18 Ar