Answered

Welcome to Westonci.ca, where curiosity meets expertise. Ask any question and receive fast, accurate answers from our knowledgeable community. Our platform provides a seamless experience for finding precise answers from a network of experienced professionals. Get quick and reliable solutions to your questions from a community of experienced experts on our platform.

If the temperature of a gas is increased from 20°C to 35°C, what is the new pressure if the original pressure was 1.2 atm? Assume that volume is constant.
Group of answer choices

A. 0.6 atm

B. 1.3 atm

C. 1.0 atm

D. 2.6 atm

Sagot :

CrystalQueen

Answer:

B.) 1.3 atm

Explanation:

To find the new pressure, you need to use Gay-Lussac's Law:

P₁ / T₁ = P₂ / T₂

In this equation, "P₁" and "T₁" represent the initial pressure and temperature. "P₂" and "T₂" represent the final pressure and temperature. After converting the temperatures from Celsius to Kelvin, you can plug the given values into the equation and simplify to find P₂.

P₁ = 1.2 atm                                    P₂ = ? atm

T₁ = 20 °C + 273 = 293 K              T₂ = 35 °C + 273 = 308 K

P₁ / T₁ = P₂ / T₂                                             <----- Gay-Lussac's Law

(1.2 atm) / (293 K) = P₂ / (308 K)                  <----- Insert values

0.0041 = P₂ / (308 K)                                   <----- Simplify left side

1.3 = P₂                                                         <----- Multiply both sides by 308

Thanks for using our service. We aim to provide the most accurate answers for all your queries. Visit us again for more insights. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Westonci.ca is your go-to source for reliable answers. Return soon for more expert insights.