Data Given:
Pressure = P = 2.5 kPa = 0.02467 atm
Temperature = T = 157 °C + 273.15 = 430.15 K
Volume = V = ?
Mass = m = 10 g
First find out moles for given amount of Argon gas,
As,
Moles = Mass / M.mass
Putting values,
Moles = 10 g / 39.94 g/mol = 0.250 moles
Now using Ideal Gas Equation,
P V = n R T
Solving for V,
V = n R T / P
Putting Values,
V = (0.25 mol × 0.0821 L.atm.mol⁻¹.K⁻¹ × 430.15 K) ÷ 0.02467 atm
Volume = 357.87 L
Answer:
The answer is A, if im not mistaken
Answer:
0.189
Explanation:
Aqueous solution only has ammonia and water in it. Assume total mass of 100 g
Meaning mass of ammonia is 18% of 100 g = 18 g
Mass of water is 82% of 100 g = 82g
Number of moles of ammonia = mass / molar mass ammonia =18/17 = 1.059
Number of moles of water = mass / molar mass water = 82/18 =4.556
Mole fraction ammonia = 1.059 / (1.059+4.556) = 0.189
Answer:
51.0 meters/second is the final speed
Round 89 to 90 then divide by 4. so its 24.