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What is the pressure exerted by 68.0 g of nitrogen trihydride gas in a 50.0L container at 30.0 C?

What is the pressure exerted by 68.0 g of nitrogen trihydride gas in a 50.0L container at 30.0 C?
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What is the pressure exerted by 68.0 g of nitrogen trihydride gas in a 50.0L container at 30.0 C?

User Matt Morrison
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Answer:

Molecular mass of NH3 = ( 14 + 3 ) = 17 g


PV = (m)/(m _(r)) RT \\ P * 50.0 * {10}^( - 6) = (68.0)/(17) * 8.314 * (30.0 + 273) \\ P = \frac{68.0 * 8.314 * 303}{17 * 50.0 * {10}^( - 6) } \\ P = 2.02 * {10}^(8) \: Pascals

User ScaleOvenStove
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