What is the resulting pressure when a sample of gas at 25°C in a 500 ml balloon with a pressure of 800 torr is changed to 75°C and a volume of 2 liters?

233.56 torr

Explanation:

We'll begin by converting celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 25 °C

Initial temperature (T₁) = 25 °C + 273

Initial temperature (T₁) = 298 K

Final temperature (T₂) = 75 °C

Final temperature (T₂) = 75 °C + 273

Final temperature (T₂) = 348 K

Next, we shall convert 2 L to mL. This can be obtained as follow:

1 L = 1000 mL

Therefore,

2 L = 2 L × 1000 mL / 1 L

2 L = 2000 mL

Finally, we shall determine the resulting pressure. This can be obtained as follow:

Initial temperature (T₁) = 298 K

Initial volume (V₁) = 500 mL

Initial pressure (P₁) = 800 torr

Final temperature (T₂) = 348 K

Final volume (V₂) = 2000 mL

Final pressure (P₂) =?

P₁V₁/T₁ = P₂V₂/T₂

800 × 500 / 298 = P₂ × 2000 / 348

400000 / 298 = P₂ × 2000 / 348

Cross multiply

P₂ × 2000 × 298 = 400000 × 348

P₂ × 596000 = 139200000

Divide both side by 596000

P₂ = 139200000 / 596000

P₂ = 233.56 torr

Therefore, the resulting pressure is 233.56 torr

the answer to your question is c

chemical digestion occurs in the stomach were hcl and pepsin forms chyme, the mouth in which salivary amylase breaks down starch to form bolus, and the small intestine specifically the duodenum.