Answer:
228.3°C
Explanation:
Data obtained from the question include:
V1 (initial volume) = 506 cm3
T1 (initial temperature) = 147°C = 247 + 273 = 420K
V2 (final volume) = 604 cm3
T2 (final temperature) =?
The gas is simply obeying Charles' law because the pressure is constant.
The final temperature of the gas can be obtained by using the Charles' law equation V1/T1 = V2/T2 This is illustrated below:
V1/T1 = V2/T2
506/420 = 604/T2
Cross multiply to express in linear form as shown:
506 x T2 = 420 x 604
Divide both side by 506
T2 = (420 x 604) /506
T2 = 501.3K
Now let us convert 501.3K to a temperature in celsius scale. This is illustrated below:
°C = K - 273
°C = 501.3 - 273
°C = 228.3°C
Therefore, the temperature of the gas when the volume of the gas is 604 cm3 is 228.3°C
N=24/12
n=2
where n= no. of moles
When substances change state there is no change in mass. so for physical changes are generally easy to reverse though the end product may not always look exactly the same as the starting material.
The reaction CO₂(g) → C(s) +O₂(g) is a decomposition reaction is true
Explanation
A Decomposition reaction is a reaction in which involve breaking down a compound into two or more simpler substances.
The reaction above is a decomposition reaction since CO₂ molecule is broken down into C (an element) and O₂ (a molecule).