2.24 liters is the volume of the gas if pressure is increased to 1000 Torr.
Explanation:
Data given:
Initial volume of the gas V1 = 2.6 liters
Initial pressure of the gas P1 = 860 Torr 1.13 atm
final pressure on the gas P2 = 1000 Torr 1.315 atm
final volume of the gas after pressure change V2 =?
From the data given above, the law used is :
Boyles Law equation:
P1V1 = P2V2
V2 = P1V1/P2
= 1.13 X 2.6/ 1.31
= 2.24 Liters
If the pressure is increased to 1000 Torr or 1.315 atm the volume changes to 2.24 liters. Initially the volume was 2.6 litres and the pressure was 860 torr.
Answer:
Advantakes= it is a renewable source, you can but it anywhere with sunlight
disatvantage= it cost a lot to place/replace, it uses a lot of different materials
Using ideal gas equation,

Here,
P denotes pressure
V denotes volume
n denotes number of moles of gas
R denotes gas constant
T denotes temperature
The values at STP will be:
P=1 atm
T=25 C+273 K =298.15K
V=663 ml=0.663L
R=0.0821 atm L mol ⁻¹
Mass of gas given=1.25 g g
Molar mass of gas given=?


Putting all the values in the above equation,

Molar mass of the gas=46.15
Answer:
not sure about 6 but 7 should be c
Explanation:
..
The standard entropy for the substances are as follows:
C6H12O2(s) = -212
<span>O2(g) = -205 </span>
<span>CO2(g) = -214 </span>
<span>H2O(l) = -70
</span>
We calculate the ∆S°r<span>eaction by the expression:
</span>∆S°rxn = ∆S°products - ∆S° reactants
∆S°rxn = (212+6x205)-(6x214+6x70)
∆S°rxn = -262 J/K ------> OPTION 3