Answer:
-1.4, -.7 .003, 3%(.03), .3, .66(2/3) .85 (7/8) 0.875, 100/50 (2)
Step-by-step explanation:
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:
1519
Step-by-step explanation:
if wrong super sooryyyyy :(
The equation is 4(x-3) -(5x+1) = 3
The next step is solving the equation is to apply the distributive property and the equation becomes 4x - 12 - 5x - 5 = 3.
So the correct answer is the third option.
28 x 12 = 336
336 - 16 = 320
320 divided by 4 = 80
80
Lights