For many purposes we can treat methane (CH) as an ideal gas at temperatures above its boiling point of -161. °C. Suppose the temperature of a sample of methane gas is raised from -13.0 °C to 17.0°C, and at the same time the pressure is changed. If the initial pressure was 0.26 kPa and the volume increased by 30.0%, what is the final pressure? Round your answer to the correct number of significant digits.

Explanation:

You can use the combined gas law:

You need to find P₂ when:

Thus, clear P₂ from the equation, subsitute and compute:

         P₂ = 0.26kPa ← answer

Since the factor P₁ has two significant figures, the result is limited to two significant figures.

idk

explanation:

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.