Answer: The initial volume is 593.76mL
Step-by-step explanation:
As you do not say anithing about the pressure, i guess that the pressure remains constant.
If the gas is an ideal gas, we have:
P*V = n*R*T
where P is pressure, n is number of moles and R is a constant.
Now, initially we have:
P*Vi = n*R*315°C
finally we have:
P*825mL = n*R*452°C
Now we can take the quiotient of those two equations and get:
(P*Vi)/(P*852mL) = (n*R*315°C)/( n*R*452°C)
Now we have:
Vi/852mL = 315/452
Vi = (315/452)*852mL = 593.76mL
So when we expand the gas at constant pressure, we increase the temperature.
Answer: 441
Step-by-step explanation:




441
Step-by-step explanation:
Simple
We will subtract
21 - 16 = 5
So 5 more students can join the class
Answer:
17.9 units is the answer
Step-by-step explanation:
points are (-7,-2) and (9,6)
Pythagorean theorem can be written as,

Rounding off,
d = 17.9 units
12 because db/ad = 3 and ab = 8
thus de+(de/3) is the answer
12 <- answer