How many moles of co2 form when 58.0 g of butane, c4h10, burn in oxygen? 2c4h10 + 13o2 → 8co2 + 10h2o a. 4 mol b. 2 mol c. 8 mol d. 10 mol

The molar mass of butane is 12 * 4 + 1 * 10 = 58 grams, so we have one mole of butane.  Because this reaction creates eight molecules of CO2 for every two molecules of butane, it creates four CO2 molecules for every butane molecule, so, because we only have one mole of butane, it creates four moles of CO2.

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.