Answer:
300K
Explanation:
Given pressure of the system decreased by 10 times which means 
Given the volume of the system increased by 5 times which means 
Given final temperature 
Let the initial temperature be 
We know that PV=nRT
As n and R are constant 
T1=300K
It must be noted that our compound contains only two components, N and O. From the given masses, the total mass of the compound should be 300 g.
Then, we divide the masses of each component by the total mass and multiply the quotients by 100% to get the % compositions
N = (222.6 g / 300 g) x 100% = 74.2%
O = (77.4 g / 300 g) x 100% = 25.8%
Answer:
Mass = 525.36 g
Explanation:
Given data:
Mass of CO₂ formed = ?
Mass of CH₄ burned = 191 g
Solution:
Chemical equation:
CH₄ + 2O₂ → CO₂ + 2H₂O
Number of moles of CH₄:
Number of moles = mass/molar mass
Number of moles = 191 g/ 16 g/mol
Number of moles = 11.94 mol
Now we will compare the moles of CH₄ and CO₂.
CH₄ : CO₂
1 : 1
11.94 : 11.94
Mass of CO₂:
Mass = number of moles × molar mass
Mass = 11.94 mol × 44 g/mol
Mass = 525.36 g
