What pressure will cause 1.70 atm and 300.0°C to increase to 350.0°C ? Assume constant volume. Reminder : Kelvin = 273 + °C *

1.85 atm

Explanation:

Initial pressure P1 = 1.70 atm

Initial temperature T1 = 300.0°C

Convert temperature in Celsius to Kelvin i.e (273 + 300.0°C) = 573K

Final pressure P2 = ?

Final temperature T2 = 350.0°C

(273 + 350.0°C) = 623K

Mathematically, pressure law states the pressure (p) of a gas is directly proportional to the absolute temperature (T).

i.e Pressure ∝ Temperature.

P1/T1 = P2/T2

1.70 atm/573K = P2/623K

P2 = (1.70 ATM x 623K) / 573K

P2 = 1059.1/573

P2 = 1.85 atm

Thus, the 1.85 atm of pressure is required.

the correct answer is option d

explanation:

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

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.