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A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37 degrees Celsius How many moles of nitrogen are in the container?
To calculate the number of moles of nitrogen gas in the container, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Convert the pressure to atm, the volume to L, and the temperature to Kelvin. Then plug in the values and solve for n.
What is the pressure exerted by 32 g of O2 in a 22.0-L container at 30.0 degrees Celsius?
The first step is to convert the mass of O2 to moles using the molar mass of O2. Then, use the ideal gas law equation (PV = nRT) to calculate the pressure. Plug in the values for volume, temperature, and the number of moles of O2 to find the pressure.
What is the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide 3 moles of nitrogen and 1 mole of hydrogen and has a total pressure of 1.05 ATM?
The total moles of gas in the container is 9 moles (5 moles CO2 + 3 moles N2 + 1 mole H2). To find the partial pressure of CO2, divide the moles of CO2 by the total moles of gas and multiply by the total pressure: (5 moles CO2 / 9 moles total gas) * 1.05 ATM = 0.5833 ATM. Therefore, the partial pressure of CO2 in the container is 0.5833 ATM.
How many moles of krypton are there in 6.11 L of the gas at 802 atm and 31 degrees celsius?
802 atmospheres? You sure? Anyway, the formula is the important thing. Use the ideal gas equation/law. pressure atm * volume Liters = moles * R * temperature Kelvin PV = nRT 31 degrees Celsius = 304.15 Kelvin (802 atm)(6.11 Liter) = n(0.08206 L*atm/mol*K)(304.15 K) 4900.22 = 24.959n = 196 moles of Krypton --------------------------------
How much heat is evolved when 50.0mL of CS2 that has density of 1.263 grams per milliliter reacts with 5.00L of chlorine gas at 2.78atm and 27 degree Celsius?
To find the heat evolved, you need to first calculate the moles of CS2 and Cl2 reacting. Then, use the stoichiometry of the reaction to determine the moles of substance reacted. Finally, use the ideal gas law to find the final volume of the gases in the reaction at the given conditions. The heat evolved can then be calculated using the heat of reaction and the moles of reactants.
What is the volume of a gas if 0.182 moles of the gas is at 1.99 arm and 83.4 degree Celsius?
The volume is 2,67 L.
The gaseous product of a reaction is collected in a 25.0-L container at 27C The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g How many moles of the gas are in the container?
You can use the ideal gas law, PV = nRT, to solve for the number of moles, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Rearrange the formula to solve for n, n = (PV) / (RT). Convert the temperature from Celsius to Kelvin (27°C + 273 = 300 K), and plug in the values to find the number of moles of the gas in the container.
A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37 degrees Celsius How many moles of nitrogen are in the container?
To calculate the number of moles of nitrogen gas in the container, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Convert the pressure to atm, the volume to L, and the temperature to Kelvin. Then plug in the values and solve for n.
How Many Moles of air are there in a 3 L container of 1 ATM pressure and 293?
0.125 moles
How many moles are there in a 3 L container at 1 ATM pressure and 293 K?
The answer is 0,125 moles.
How many moles of air are there in a 3 L container a 1 ATM pressure and 293 K?
0.125 moles
When a container is filled with 3 moles of H 2 moles of O and 1 mole of N the pressure in the container is 8.7 ATM. The partial pressure of O 2 is?
impossible to calculate
How manymoles od propane are in a presure container that has 2.55Kg of propane C3H8molar mass of C3H844.11gmol?
To find the number of moles of propane in the container, first convert the mass of propane to grams: 2.55 kg = 2550 grams Next, calculate the number of moles using the molar mass of propane: Molar mass of C3H8 = 44.11 g/mol Number of moles = 2550 g / 44.11 g/mol = 57.86 moles Therefore, there are 57.86 moles of propane in the pressure container.
How many moles of N2 are there at a temperature of 20 degrees Celsius 1 ATM pressure if the gas occupies 44 Liters?
The answer is 1,83 moles.
What would the effect on temperature and volume be if you changed the number of moles of gas in a container?
In a container the volume remain constant but the pressure increase.
If 4 moles of gas are added to a container that already holds 1 mole of gas the pressure inside the container what due to the change in the amount of gas?
To answer this question you first need to know how big the container is. What is the volume of the container?
How many moles of fluorine gas are there in 564 ml of fluorine gas at A degrees Celsius 145 KP?
Number of moles is 9,8355/T (T in kelvin).
