A piston is holding 125 mL of gases at a temperature of 300 K and a pressure of 2.39 atm. What is the volume of the gases if the temperature is increased to 500K and the pressure falls to 2.15 atm

231.59 mL

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 125 mL

Initial temperature (T₁) = 300 k

Initial pressure (P₁) = 2.39 atm

Final temperature (T₂) = 500 k

Final pressure (P₂) = 2.15 atm

Final volume (V₂) =..?

The new volume of the gas (V₂) can be obtained by using the combined gas equation as shown below:

P₁V₁ /T₁ = P₂V₂ /T₂

2.39 × 125 /300 = 2.15 × V₂ /500

Cross multiply

300 × 2.15 × V₂ = 2.39 × 125 × 500

645 × V₂ = 149375

Divide both side by 645

V₂ = 149375/645

V₂ = 231.59 mL

Therefore, the new volume of the gas is 231.59 mL

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

answer: they produce more slow than unicellular organisms.