A sample of gas starts at 1.2 atm, 107 degrees C° and 1,540 mL what is the volume in mL if the temps true increases to 110 C° and the pressure increases to 3.6 atm?

517ml

Explanation:

Given that:

Volume of gas V1 = 1540mL

Temperature T1 = 107°C

Convert Celsius to Kelvin

(107°C + 273 = 380K)

Initial Pressure P1 = 1.2 atm

Final Volume V2 = ?

Final temperature T2 = 110°C

(110°C + 273 = 383K)

Final pressure = 3.6 atm

Then, apply the general gas equation

(P1V1)/T1 = (P2V2)/T2

(1.2 x 1540)/380 = (3.6 x V2)/383

1848/380 = 3.6V2/383

4.86 = 0.0094V2

Divide both sides by 0.0094

4.86/0.0094 = 0.0094V2/0.0094

517 = V2

Thus, the final volume is 517ml

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

answer: any goods being imported from another country may be subject to issued by the federal government are tariffs

explanation:  

tariffs are a tax on anything that are imported from abroad. government use them to protect and boost their local industries and the thought is that they encourage consumers to buy local instead of importing and they will hope will protect jobs and economy in the country that implements them