Answer :
We start by noting the conversion factor between atmospheres and kilopascals, namely:
[tex]$$
1 \text{ atm} = 101.325 \text{ kPa}.
$$[/tex]
Given that the pressure is [tex]$2.42$[/tex] atm, we convert it to kilopascals by multiplying by the conversion factor:
[tex]$$
P_{\text{kPa}} = 2.42 \, \text{atm} \times 101.325 \, \frac{\text{kPa}}{\text{atm}}.
$$[/tex]
Calculating the multiplication:
[tex]$$
P_{\text{kPa}} \approx 245.2065 \text{ kPa}.
$$[/tex]
This result is approximately [tex]$245$[/tex] kPa when rounded. Therefore, the pressure of the gas is about
[tex]$$245 \text{ kPa}.$$[/tex]
[tex]$$
1 \text{ atm} = 101.325 \text{ kPa}.
$$[/tex]
Given that the pressure is [tex]$2.42$[/tex] atm, we convert it to kilopascals by multiplying by the conversion factor:
[tex]$$
P_{\text{kPa}} = 2.42 \, \text{atm} \times 101.325 \, \frac{\text{kPa}}{\text{atm}}.
$$[/tex]
Calculating the multiplication:
[tex]$$
P_{\text{kPa}} \approx 245.2065 \text{ kPa}.
$$[/tex]
This result is approximately [tex]$245$[/tex] kPa when rounded. Therefore, the pressure of the gas is about
[tex]$$245 \text{ kPa}.$$[/tex]
