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:
3524.4 g
Step-by-step explanation:
- Use formula: Density = Mass/Volume
- Mass= Density * Volume
Answer: 3/4 or 75%
Step-by-step explanation:
Answer:
The null hypo would be the difference is greater than 0
so the alternate hypothesis would be less than or equal to 0
H1: µd ≤ 0
