Answer:
1. 136 °C.
2. 0.21 atm.
Explanation:
1. Determination of the new temperature in °C.
Initial volume (V1) = 1.35L
Final volume (V2) = 1.95L
Initial temperature (T1) = 283 K
Final temperature (T2) =...?
Using the Charles' law equation, the new temperature of the gas can be obtained as follow:
V1 /T1 = V2 /T2
1.35/283 = 1.95/T2
Cross multiply
1.35 × T2 = 283 × 1.95
1.35 × T2 = 551.85
Divide both side by 1.35
T2 = 551.85/1.35
T2 = 408.8 ≈ 409 K
Finally, we shall convert 409 K to °C. This can be obtained as follow:
T (°C) = T(K) – 273
T(K) = 409 K
T (°C) = 409 – 273
T (°C) = 136 °C
Therefore, the new temperature of the gas is 136 °C.
2. Determination of the new pressure.
Initial pressure (P1) = 1.34 atm
Initial volume (V1) = 267 mL
Final volume (V2) = 1.67 L
Final pressure (P2) =.?
Next, we shall convert 1.67 L to millilitres (mL). This can be obtained as follow:
1 L = 1000 mL
Therefore,
1.67 L = 1.67 L × 1000 mL / 1 L
1.67 L = 1670 mL
Therefore, 1.67 L is equivalent to 1670 mL.
Finally, we shall determine the new pressure of the gas as follow:
Initial pressure (P1) = 1.34 atm
Initial volume (V1) = 267 mL
Final volume (V2) = 1670 mL
Final pressure (P2) =.?
P1V1 = P2V2
1.34 × 267 = P2 × 1670
357.78 = P2 × 1670
Divide both side by 1670.
P2 = 357.78 / 1670
P2 = 0.21 atm.
Therefore, the new pressure of the gas is 0.21 atm.
