Answer:
1.99 atm
Explanation:
Step 1:
Data obtained from the question. This include the following:
Initial pressure (P1) = 0.520 atm
Initial temperature (T1) = 26.2°C
Initial volume (V1) = 15.4L
Final temperature (T2) = constant = 26.2°C
Final volume (V2) = 4.02L
Final pressure (P2) =..?
Step 2:
Determination of the new pressure of the gas.
Since the temperature of the gas is constant, it means the gas is obeying Boyle's law. Thus, the new pressure of the gas can be obtained by applying the Boyle's law equation as shown below:
P1V1 = P2V2
0.520 x 15.4 = P2 x 4.02
Divide both side by 4.02
P2 = (0.520 x 15.4) / 4.02
P2 = 1.99 atm
Therefore, the new pressure of the gas is 1.99 atm
Explanation:
Heat energy lost by metal = Heat energy gained by water.
(0.00138kg) * c * (99.6-31.6) = (0.006050kg) * 4.148 * (31.6-22.1)
c = 2.541J/kg°C
Answer:- 0.158 moles
Solution:- Moles are calculated on dividing the grams by the molar mass.
25.0 grams of 
are given and we are asked to calculate the moles.
For this we need the molar mass so let's calculate it first.
Molar mass is the sum of atomic masses of all the atoms present in the molecule.
Molar mass = 
= 158.036 gram per mol
Now, we will divide the given grams by molar mass to get the moles and the set is shown as:
= 
So, there are 0.158 moles of .
