Astudent collects 285ml of nitrous oxides gas at 15.8°c and a pressure of 1.05atm. the next day, the same sample occupies a volume of 292ml at a temperature of 11.2°c. what is the new pressure in kpa?

1.01 atm  

Step-by-step explanation:

To solve this problem, we can use the Combined Gas Laws:

p₁V₁/T₁ = p₂V₂/T₂     Multiply each side by T₂

p₁V₁T₂ = p₂V₂           Divide each side by V₂

     p₂ = p₁ × V₁/V₂ × T₂/T₁

Data:

p₁ = 1.05 atm; V₁ = 285 mL; T₁ = 15.8 °C

p₂ = ?;            V₂ = 292 mL; T₂ =  11.2 °C

Calculations:

(a) Convert temperatures to kelvins

T₁ = (15.8+273.15) K = 288.95 K

T₂ = (11.2+273.15) K = 284.35 K

(b) Calculate the pressure

p₂ = 1.05 atm× (285/292) × (284.35/288.95)  

   = 1.05 atm × 0.9760 × 0.9840

   = 1.01 atm

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)

the answer is b. dilution