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 atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.