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:
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Answer:
49 and 58
Step-by-step explanation:
pls brainliest
Answer:
y= 1/4x+5
Step-by-step explanation:
y=mx+c
to calculate gradient: change in y/change in x
-3/-12 = 0.25
y = 1/4x+c
4 * 1/4 = 1
6-1 = 5
c= 5
Totally:
y= 1/4x+5
