Question

What is the approximate energy required to raise the temperature of 1.00 L of hydrogen by 90 °C? The pressure is held constant and equal to 1 atm.

Answer 1

Q = 116.8 J

Step-by-step explanation:

Here given that the temperature of 1 L hydrogen is increased by 90 degree C at constant pressure condition.

So here we will have

`Q = n C_p \Delta T`

here we know that

n = number of moles

`n = (1)/(22.4)`

`n = 0.0446`

for ideal diatomic gas molar specific heat capacity at constant pressure is given as

`C_p = (7)/(2)R`

now we have

`Q = (0.0446)((7)/(2)R)(90)`

`Q = 116.8 J`