Answer:
B. 4.76 atm
Explanation:
[tex]P_1[/tex] = Initial pressure = 3.8 atm
[tex]T_1[/tex] = Initial temperature = [tex]25+273.15\ \text{K}[/tex]
[tex]P_2[/tex] = Final pressure
[tex]T_2[/tex] = Final temperature = [tex]100+273.15\ \text{K}[/tex]
From Gay Lussac's law we have
[tex]\dfrac{P_2}{P_1}=\dfrac{T_2}{T_1}\\\Rightarrow P_2=P_1\dfrac{T_2}{T_1}\\\Rightarrow P_2=3.8\times\dfrac{100+273.15}{25+273.15}\\\Rightarrow P_2=4.76\ \text{atm}[/tex]
The pressure inside the can would be [tex]4.76\ \text{atm}[/tex].
