1. A steel cylinder with a volume of 15.0L is filled with 80.4g of nitrogen gas at 25C. What is the pressure, in atmospheres, of the N2 gas in the cylinder?
2.When sensors in a car detect a collision, they cause the reaction of sodium azide, NaN3, which generates nitrogen gas to fill the air bags within 0.03 s. How many liters of N2 are produced at STP if the air bag contains 145g of NaN3 ?
2NaN3(s)→2Na(s)+3N2(g)
3. If the He injected into the abdomen produces a pressure of 14mmHg and a volume of 3.0L at 25C, how many grams of He were used?
To solve these problems, we need to use the ideal gas law equation, which is PV = nRT. In this equation, P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
1. To find the pressure of the nitrogen gas in the cylinder, we need to convert the volume from liters to cubic meters and the temperature from Celsius to Kelvin. We can use the given mass of nitrogen gas to find the number of moles using the molar mass of nitrogen gas (28.0134 g/mol). We can then substitute the values into the ideal gas law equation to find the pressure in atmospheres.
2. To find the volume of nitrogen gas produced at STP (Standard Temperature and Pressure), we need to convert the given mass of NaN3 to moles using its molar mass (65 g/mol). From the balanced chemical equation, we know that 2 moles of NaN3 produce 3 moles of N2. We can use the mole ratio and the ideal gas law equation to calculate the volume of N2 gas in liters.
3. To find the mass of helium injected, we need to convert the pressure from mmHg to atmospheres and the volume from liters to cubic meters. Then using the given pressure, volume, and temperature in Kelvin, we can rearrange the ideal gas law equation to solve for the number of moles. Finally, we can convert the moles of helium gas to grams using its molar mass (4.0026 g/mol).
Keep in mind to always convert the units and use the appropriate gas constant (R) for the units used.