A gas sample with a volume of 5.3 l has a pressure of 735 mm hg at 28 c. What is the sample if the volume remains at 5.3 l but the temperature rises to 86 c

876.63 mmHg

Explanation:

Step 1:

Data obtained from the question:

Initial volume (V1) = 5.3 L

Initial pressure (P1) = 735 mmHg

Initial temperature (T1) = 28°C

Final volume (V2) = constant i.e the same as the initial volume (5.3L)

Final temperature (T2) = 86°C

Final pressure (P2) =..?

Step 2:

Conversion of celsius temperature to Kelvin temperature. This is illustrated below:

Temperature (Kelvin) = temperature (celsius) + 273

Initial temperature (T1) = 28°C

Initial temperature (T1) = 28°C +273 = 301K

Final temperature (T2) = 86°C

Final temperature (T2) = 86°C + 273 = 359K

Step 3:

Determination of the new pressure of the gas. This is illustrated below:

Since the volume of the gas is constant, the new pressure of the gas can be obtained by the equation below:

P1/T1 = P2/T2

Initial pressure (P1) = 735 mmHg

Initial temperature (T1) = 301K

Final temperature (T2) = 359K

Final pressure (P2) =..?

P1/T1 = P2/T2

735/301 = P2/359

Cross multiply to express in linear form

301 x P2 = 735 x 359

Divide both side by 301

P2 = (735 x 359)/301

P2 = 876.63 mmHg

Therefore, the new pressure of the gas is 876.63 mmHg

why is cellular respiration important for homeostasis?

it changes food into energy that the organism can use.

which of the following is most likely to happen if a cell is not able to divide?

the cell will not be replaced when it is damaged.

explanation:

answer; the numbers of valence electrons in the acetic acid molecule (ch3co2h) is 24;