The given question is incomplete. The complete question is :
Gaseous butane reacts with gaseous oxygen gas to produce gaseous carbon dioxide and gaseous water . If 1.31g of water is produced from the reaction of 4.65g of butane and 10.8g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.
Answer: 28.0 %
Explanation:
To calculate the moles :
According to stoichiometry :
13 moles of 
require 2 moles of butane
Thus 0.34 moles of will require=
of butane
Thus is the limiting reagent as it limits the formation of product and butane is the excess reagent.
As 13 moles of give = 10 moles of 
Thus 0.34 moles of give =
of
Mass of 
The percent yield of water is 28.0 %
The main functions of the cell wall are to provide structure, support, and protection for the cell.
Answer:
The temperature of the methanol will increase more rapidly.
Explanation:
The premise of your question is incorrect. Methanol has an OH group, so there ARE hydrogen bonds among methanol molecules.
However, the specific heat capacity of methanol is 2.53 J°C⁻¹g⁻¹, while that of water is 4.18 J°C⁻¹g⁻¹.
Thus, it takes 65 % more heat energy to raise the temperature of a given mass of water by 1 °C than it does to raise the temperature of an equal mass of methanol by the same amount.
The two samples are receiving heat energy at the same rate, so the methanol will heat up faster than the water.
