Determine which law is appropriate for solving the following problem. what temperature will 215 ml of a gas at 20°c and 1 atm pressure attain when it is subject to 1.5 atm of pressure? what law is used: combined gas law, charles law, or boyles law?

The Combined Gas Law

Explanation:

Let’s compare the two conditions.

p₁ = 1     atm; V₁ = 215 mL; T₁ = 20 °C

p₂ = 1.5 atm; V₂ = 215 mL; T₂= ?

The only variables are pressure and temperature.

The most appropriate law would be Gay-Lussac’s Law (p₁/T₁ = p₂/T₂), but that’s not an option.

The only other option involving p and T is the Combined Gas Law:

p₁V₁/T₁ = p₂V₂/T₂

Since V₂ = V₁, we can write

p₁V₁/T₁ = p₂V₁/T₂     Divide both sides by V₁

    p₁/T₁= p₂/T₂         Multiply both sides by T₂

p₁T₂/T₁ = p₂               Multiply both sides by T₁

    p₁T₂= p₂T₁            Divide both sides by p₁

      T₂ = T₁ × p₂/p₁

Now, convert your temperature to kelvins, insert the values into the formula, and calculate the new temperature.

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o