A rigid container contains 1 mole of H2 at 300 K and 1 bar. If H2...

 

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A rigid container contains 1 mole of H2 at 300 K and 1 bar. If H2 can be considered as an ideal gas, what is the total amount of heat required to increase its pressure from 1 bar to 2.5 bar (You need to consider the temperature dependence of the molar heat capacity of H2; i.e., Cp=a+bT+cT²+dT³)? If the autoignition temperature of H2 is 500 °C, are we still safe when we reach 2.5 bar? Which value would you calculate for the total amount of heat to increase the pressure to 2.5 bar if you have used a constant heat capacity for H2? A rigid container contains 1 mole of H2 at 300 K and 1 bar. If H2 can be considered as an ideal gas, what is the total amount of heat required to increase its pressure from 1 bar to 2.5 bar (You need to consider the temperature dependence of the molar heat capacity of H2; i.e., Cp=a+bT+cT²+dT³)? If the autoignition temperature of H2 is 500 °C, are we still safe when we reach 2.5 bar? Which value would you calculate for the total amount of heat to increase the pressure to 2.5 bar if you have used a constant heat capacity for H2?

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