How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127°C? A. 89.6 mol B. 6.38 mol C. 0.24 mol D. 0.77 mol

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How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127°C? A. 89.6 mol B. 6.38 mol C. 0.24 mol D. 0.77 mol

Chemistry
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You're going to have to use the formula PV=nRT P is the pressure V is your volume n is the number of moles R is the ideal gas constant T is your temperature
The Pressure would have to be in atmospheres in order to use 0.0821 as your R value and your temperature has to be in Kelvin instead of celcius
202.6kPa is equal to 2.0atm so thats your pressure that you can use in the formula 127+273=400K so you can use 400K as your temperature

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P=2.0atm V=4.0L n=unknown R=0.0821L-atm/mole-K T=400K Put them into the formula to solve for n
\[\frac{ pV }{ RT } = n \]

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