its false as only gas has that ability to do so
The question is incomplete.
This is the complete question:
Consider equimolar samples of different ideal gases at the same volume and temperature. Gas A has a higher molar mass than gas B.
Compare the pressures. Compare the rms speeds. Compare the average kinetic energies.
pressure: A = B
RMS: A < B
kinetic energies: A = B
You can deal with this part of the question on the basis of Avogaro's principle which stated that equal volumes of gases at same temperature and pressure have the same number of particles (molecules).
Also, kinetic theory of gases postulates that the particles of gas are quited separated and in consequence the volume occupied by the particles of a gas is meaningless and does not influence the total volume occupied by a fixed number of particles.
Also, you can use the equation of ideal gases pV = nRT, from which p = nRT/V. if n, T, and V are fixed, then p is fixed.
The three approaches leads to the same conclusion.
Then, pressure of gas A is equal to pressure of gas B.
RMS stands for root mean square speed.
It is the room mean square speed of the particles of a gas.
the RMS is related with the temperature of the gas and the molar mass per this equation:
RMS = √(3RT/M), where R is the universal constant of gases, T is the absolute temperature and M is the molar mass.
Then, the greater the molar mass, the lower the RMS, which permits you conclude that the RMS of gas A is less than the RMS of the gas B.
3) kinetic energy
Temperature is a measure of the kinetic energy.
Equal temperatures of the gas means equal kinetic energies.
The Kinetic Molecular Theory states that the average energy of molecules is proportional to absolute temperature.
So, you conclude that the same amount of gases, at the same temperature, contain equal kinetic energies.
The bases like chloride, hydroxides and methoxide ions can accept a proton from an acid because, they are more attracted to a proton in the negative charged form.
Formic acid is a carboxylic acid having the form HCOOH . The pKa value of formic acid is 3.74. Thus the acidity of formic acid is greater than that of acetic acid and common alcohols.
According to Bronsted- Lowry concept of acids and bases, acids are substances able to donate protons to the bases and bases accept protons from acids.
Formic acid upon deprotonation forms HCOO⁻ and it is called formate ion. Substances with higher basicity remove the protons from the carboxylic part of formic acid.
Bases containing a negative charge are highly active and will easily remove a proton from acids. Thus, bases such as chloride, hydroxides and methoxide ions remove the H from HCOOH to form their protonated forms HCl, H₂O and CH₃OH respectively.
Other substance such as CH₃OH and CH₃NH₂ are less basic and cannot accept a proton from highly acidic HCOOH . Hence, options a, d, e are correct.
To find more about Bronsted- Lowry concept, refer the link below:
Your question is incomplete. But your complete question probably was:
Which of the following bases can remove a proton from formic acid in a reaction that favors products? Check all that apply.
c. acetic acid
e. methoxide ion