A sample of helium gas has a volume of 900. milliliters and a pressure of 2.50 atm at 298 K. what is the new pressure when the temperature is changed to 336K and the Volume is decreased to 450. milliliters?

a- 0.177
b- 14.1
c- 5.64
d- 4.43

(p1v1)/T1 = (p2v2)/T2

Post your work if you get stuck.

To solve this problem, we can use the combined gas law equation:

(P1 * V1) / T1 = (P2 * V2) / T2

P1 = 2.50 atm (initial pressure)
V1 = 900 mL (initial volume)
T1 = 298 K (initial temperature)
P2 = ? (new pressure)
V2 = 450 mL (new volume)
T2 = 336 K (new temperature)

Now, let's plug in the given values into the equation:

(2.50 atm * 900 mL) / 298 K = (P2 * 450 mL) / 336 K

Simplifying the equation:

2250 atm mL / 298 K = (P2 * 450 mL) / 336 K

Cross-multiplying:

(2250 atm mL * 336 K) = (P2 * 450 mL * 298 K)

756000 atm mL K = 134100 P2 mL K

Dividing both sides by 134100 P2 mL K:

P2 = (756000 atm mL K) / (134100 mL K)
P2 ≈ 5.64 atm

Therefore, the new pressure when the temperature is changed to 336 K and the volume is decreased to 450 mL is approximately 5.64 atm.

Answer: c- 5.64

To solve this problem, we can use the combined gas law formula:

P₁V₁/T₁ = P₂V₂/T₂

where:
P₁ = initial pressure
V₁ = initial volume
T₁ = initial temperature
P₂ = final pressure (what we're trying to find)
V₂ = final volume (given as 450 mL)
T₂ = final temperature (given as 336 K)

Let's plug in the known values into the formula:

P₁ = 2.50 atm
V₁ = 900 mL
T₁ = 298 K
V₂ = 450 mL
T₂ = 336 K

Now we rearrange the formula to isolate P₂:

P₂ = (P₁V₁T₂) / (V₂T₁)

Let's substitute the values and calculate:

P₂ = (2.50 atm * 900 mL * 336 K) / (450 mL * 298 K)
= (2.25 * 10^5 atm·mL·K) / (1.34 * 10^5 mL·K)
≈ 1.68 atm

Therefore, the new pressure when the temperature is changed to 336 K and the volume is decreased to 450 mL is approximately 1.68 atm.

Hence, the correct answer is not provided in the options.