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This is a chemical calculation. You need 9.752dm3 for store it.

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9y ago

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What volume is needed to store 0.050 moles of helium gas at 202.6 kPa and 400 K?

The volume is 0,82 L.


What volume is needed to store 0.80 moles helium gas at 204.6 kpa and 300 k?

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What volume is needed to store 0.08 moles of helium gas at 204.67 KP and 300 k?

This is very easy. you need 9.752l for that.


What volume is needed to store 0.80 moles of helium gas at 204.6 KP and 300 k?

Use the equation PV=nRT. You need 9.75 l containerfor store.


What is the volume of the container needed to store 0.8 moles of argon gas at 5.3 ATM and 227C?

To find the volume of gas, you can use the ideal gas law equation: PV = nRT. Plug in the values for pressure (5.3 ATM), temperature (227°C converted to Kelvin by adding 273), moles of gas (0.8), and the ideal gas constant (0.0821 L·atm/mol·K). Solve for V (volume) to find the volume of the container needed to store 0.8 moles of argon gas at those conditions.


What volume is needed to store 0.80 moles of helium gas at 204.6 kPa and 300 K?

Using the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature in Kelvin, you can solve for V. Rearranging the equation to solve for V, you get V = (nRT)/P. Plugging in the values n = 0.80 moles, R = 8.31 J/(K*mol), T = 300 K, and P = 204.6 kPa (convert to Pa first), you can calculate the volume needed.


What volume is needed to store .80 moles of helium gas at 204.6 kpa and 300 kelvin?

First let's convert 204.6kPa to atm: 204.6 / 101.3 = 2.02atm. Now, use PV = nRT: (2.02)(V) = (0.80)(0.0821)(300), solve for V to get 9.75L, so a 10L container would work just fine.


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