Answer:
45.03 mL.
Explanation:
- We can use the general law of ideal gas: <em>PV = nRT.</em>
where, P is the pressure of the gas in atm.
V is the volume of the gas in L.
n is the no. of moles of the gas in mol.
R is the general gas constant,
T is the temperature of the gas in K.
- If n and P are constant, and have different values of T and V:
<em>(V₁T₂) = (V₂T₁).</em>
V₁ = 50.0 mL, T₁ = 119ºC + 273 = 392 K,
V₂ = ??? mL, T₂ = 80ºC + 273 = 353 K.
∴ V₂ = (V₁T₂)/(T₁) = (50.0 mL)(353 K)/(392 K) = 45.03 mL.
Different forms of matter have different melting/boiling points. For example, at 100 degrees Celsius, H2O (water) will turn from lliquid to gas. But NaOH (table salt) doesn't even go from solid to liquid until some 800 degrees Celsius. So, in order to figure out which state matter is at 35 Celsius, you'd have to be more specific about what kind of matter...
Answer:
He should have not been running through the lab. If he wasn't running he might not have broke the beaker. Whatever was in the beaker wasn't safe.
Explanation:
Can I get brainliest?
To determine the molar mass of the unknown gas, we use Graham's Law of Effusion where it relates the effusion rates of two gases with their molar masses. It is expressed as r1/r2 = √M2/M1. We calculate as follows:
Let 1 = argon gas 2 = unknown gas
r2 = 0.91r1r1/r2 = 1/0.91
1/0.91 = √M2/M1 = √M2/40M2 = 48.30 g/mol