Since this has to do with titration, the measured volume of NaOH used would be less than the actual volume used because some of the unused NaOH would cling to the sides of the buret and therefore wouldn't factor into the measurement
Hope this helps
There has to be a double bond then you put the rest into lone pairs
Answer:
1807.24L
Explanation:
Using combined gas law equation:
P1V1/T1 = P2V2/T2
Where;
P1 = pressure on Earth
P2 = Pressure on Mars
V1 = volume on Earth
V2 = volume on Mars
T1 = temperature on Earth
T2 = temperature on Mars
According to the information provided of the balloon in this question;
P1 = 1 atm
P2 = 4.55 torr = 4.55/760 = 0.00599atm
V1 = 14.5L
V2 = ?
T1 = 19°C = 19 + 273 = 292K
T2 = -55°C = -55 + 273 = 218K
Using P1V1/T1 = P2V2/T2
1 × 14.5/292 = 0.00599 × V2/218
14.5/292 = 0.00599V2/218
Cross multiply
14.5 × 218 = 292 × 0.00599V2
3161 = 1.74908V2
V2 = 3161 ÷ 1.74908
V2 = 1807.24L
Answer:
Making oxygen
Oxygen can be made from hydrogen peroxide, which decomposes slowly to form water and oxygen:
hydrogen peroxide → water + oxygen
2H2O2(aq) → 2H2O(l) + O2(g)
The rate of reaction can be increased using a catalyst, manganese(IV) oxide. When manganese(IV) oxide is added to hydrogen peroxide, bubbles of oxygen are given off.
Apparatus arranged to measure the volume of gas in a reaction. Reaction mixture is in a flask and gas travels out through a pipe in the top and down into a trough of water. It then bubbles up through a beehive shelf into an upturned glass jar filled with water. The gas collects at the top of the jar, forcing water out into the trough below.
To make oxygen in the laboratory, hydrogen peroxide is poured into a conical flask containing some manganese(IV) oxide. The gas produced is collected in an upside-down gas jar filled with water. As the oxygen collects in the top of the gas jar, it pushes the water out.
Instead of the gas jar and water bath, a gas syringe could be used to collect the oxygen.
