Answer:
ΔU° = 56.0 J
Explanation:
Step 1: Given data
- Work done to compress the gas (w): 83.0 J (When work is done on the gas, w is positive).
- Heat given off to the surroundings (q): -27.0 J (When heat is released to the surroundings, q is negative)
Step 2: Calculate the change in the internal energy of the gas (ΔU°)
The internal energy of a gas is the energy contained within it. We can calculate it using the following expression.
ΔU° = q + w
ΔU° = -27.0 J + 83.0 J
ΔU° = 56.0 J
Answer:
10B has 18.9%
11B has 81.1%
Explanation:Please see attachment for explanation
First, we need to get n1 (no.of moles of water ): when
mass of water = 0.0203 g and the volume = 1.39 L
∴ n1 = mass / molar mass of water
= 0.0203g / 18 g/mol
= 0.00113 moles
then we need to get n2 (no of moles of water) after the mass has changed:
when the mass of water = 0.146 g
n2 = mass / molar mass
= 0.146g / 18 g/ mol
= 0.008 moles
so by using the ideal gas formula and when the volume is not changed:
So, P1/n1 = P2/n2
when we have P1 = 1.02 atm
and n1= 0.00113 moles
and n2 = 0.008 moles
so we solve for P2 and get the pressure
∴P2 = P1*n2 / n1
=1.02 atm *0.008 moles / 0.00113 moles
= 7.22 atm
∴the new pressure will be 7.22 atm
