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.
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Rate = 40/16 = 10/4 = 5/2 = 2.5 meters/second
Unit rate = ratio where denominator is 1 = 2.5/1 meters/second
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Answer:
34 players
Step-by-step explanation:
40.00%
=0.4
0.4*85
=34
Answer:
A. 201.6 = 11.2f
Step-by-step explanation:
we solve for each unknown to verify which equality will require the division property:
#A. 201.6 = 11.2f
Hence, division property used.
#B. 35.4=Z ÷ 3.1
Hence, multiplication property used.
#C. t/3.2=15.1
Hence, multiplication property used.
#D. 201.6 = 11.2+c
Hence, subtractionproperty used.
The answer is 2/4 I believe
