If a gas's temperature doubles and its volume remains constant, then what happens to its pressure?
1 answer:
Answer : The pressure become doubles.
Explanation :
Gay-Lussac's Law : It is defined as the pressure of the gas is directly proportional to the temperature of the gas at constant volume and number of moles.
or,
where,
= initial pressure
= final pressure
= initial temperature
= final temperature =
Now put all the given values in the above equation, we get:
From this we conclude that, as the temperature of gas doubles then the pressure of gas become doubles because pressure is directly proportional to the temperature of gas.
Hence, the pressure become doubles.
You might be interested in
Answer:
0.187M
Explanation:
1)Identify the atoms that are participating in a covalent bond.
2)Draw each atom by using its element symbol. The number of valence electrons is shown by placing up to two dots on each side of the element symbol, with each dot representing a single valence electron.
3)Predict the number of covalent bonds each atom will make using the octet rule.
4)Draw the bonding atoms next to each other, showing a single covalent bond as either a pair of dots or a line representing a shared valence electron pair. If the molecule forms a double or triple bond, use two or three lines to represent the shared electron pairs, respectively.
2)Draw each atom by using its element symbol. The number of valence electrons is shown by placing up to two dots on each side of the element symbol, with each dot representing a single valence electron.
3)Predict the number of covalent bonds each atom will make using the octet rule.
4)Draw the bonding atoms next to each other, showing a single covalent bond as either a pair of dots or a line representing a shared valence electron pair. If the molecule forms a double or triple bond, use two or three lines to represent the shared electron pairs, respectively.