Question

Anyone good there at chemistry? Please help me with this problem​

Answer 1

19.5°C (nearest tenth)

Step-by-step explanation:

When a gas is trapped inside a container whose volume cannot change, the pressure is directly proportional to the Kelvin temperature.

Gay Lussac's Law

`\sf (P_1)/(T_1)=(P_2)/(T_2)`

where:

• P₁ is the initial pressure.
• T₁ is the initial temperature.
• P₂ is the final pressure.
• T₂ is the final temperature.

Temperature must be in kelvins (K).

To convert Celsius to kelvins, add 273.15.

Given values:

• P₁ = 4.882 atm
• P₂ = 4.690 atm
• T₂ = 8 C = 8 + 273.15 = 281.15 K

Substitute the given values into the equation and solve for T₁:

`\implies \sf (P_1)/(T_1)=(P_2)/(T_2)`

`\implies \sf (4.882)/(T_1)=(4.690)/(281.15)`

`\sf \implies \sf T_1=(4.882 \cdot 281.15)/(4.690)`

`\sf \implies \sf T_1=(1372.5743)/(4.690)`

`\sf \implies T_1=292.6597655...\:K`

To convert kelvins to Celsius, subtract 273.15:

`\sf \implies T_1=292.6597655...-273.15=19.5097...^(\circ)C`

`\sf \implies T_1=19.5^(\circ)C\;(nearest\;tenth)`

Therefore, the temperature of the previous day was 19.5°C (nearest tenth).