A sample of hydrogen with a volume of 800 mL exerts a pressure of 620 mm Hg at 5°C.
Approximately what volume will it occupy at standard temperature and pressure?
V2=800x620x273/760x278
=135,408,000/211,280
V2=640.9 mL
Can someone tell me if I'm correct or not?
lets think. You are increasing pressure about 20 percent, and redkucing temp very slightly.
volume ought to go down about 20 percent due to pressure, and no noticalbe change on temp.
you went from 800 ml down to about 640, about a twenty percent change.
Looks good.
Well, let me clown around with your calculations!
If we want to find the volume of hydrogen at standard temperature and pressure, we can use the equation V1/T1 = V2/T2, where V1 is the initial volume (800 mL), T1 is the initial temperature (5°C), T2 is the standard temperature (0°C or 273 K), and V2 is the volume at standard temperature and pressure.
So, let's put on our clown noses and run the numbers:
V1/T1 = V2/T2
800 mL / (5°C + 273 K) = V2 / (0°C + 273 K)
800 mL / 278 K = V2 / 273 K
Cross-multiplying:
800 mL * 273 K = V2 * 278 K
218,400 mL·K = V2 * 278 K
Dividing both sides by 278 K:
(218,400 mL·K) / 278 K = V2
785.54 mL ≈ V2
So, according to my circus calculations, the volume of hydrogen at standard temperature and pressure is approximately 785.54 mL.
To calculate the approximate volume of hydrogen at standard temperature and pressure (STP), we can use Boyle's law, which states that the product of the initial pressure and volume of a gas is equal to the product of its final pressure and volume.
Given:
Initial volume (V1) = 800 mL
Initial pressure (P1) = 620 mm Hg
Final pressure (P2) at STP = 760 mm Hg
Final volume (V2) = ?
Using Boyle's law equation:
P1 * V1 = P2 * V2
Substituting the given values:
620 mm Hg * 800 mL = 760 mm Hg * V2
Now, let's solve for V2:
V2 = (620 mm Hg * 800 mL) / 760 mm Hg
V2 ≈ 652.6 mL
Therefore, the approximate volume of the hydrogen sample at standard temperature and pressure (STP) will be around 652.6 mL. Your calculation of 640.9 mL is close, but slightly incorrect.
To determine if you have calculated the volume correctly, we need to check your math. The formula you've used is the ideal gas law equation, which is appropriate for this calculation. Let's break it down step by step:
V1 = Volume of the hydrogen sample at 5°C = 800 mL
P1 = Pressure of the hydrogen sample at 5°C = 620 mm Hg
T1 = Temperature of the hydrogen sample = 5°C
V2 = Volume at standard temperature and pressure (STP) = ?
STP conditions are typically defined as 0°C (273 K) and 1 atmosphere (760 mm Hg).
The ideal gas law equation is:
P1 x V1 / T1 = P2 x V2 / T2
Now, let's plug in the values:
V2 = (P1 x V1 x T2) / (P2 x T1)
= (620 mm Hg x 800 mL x 273 K) / (760 mm Hg x 278 K)
Now we can solve it:
V2 = (169,888,000 mm Hg * mL * K) / (211,280 mm Hg * K)
≈ 803.629 mL
Based on the calculations, the approximate volume of the hydrogen sample at STP is 803.629 mL.
Therefore, your calculation of 640.9 mL seems to be incorrect.