Water is liquid at room temperature
Answer:
If a pure compound is distilled, the temperature of the head will be compared to the temperature of the pot. However, if there is an impurity present that strongly interacts with the molecules of the liquid, then the temperature must be increased to increase the vapor pressure of the liquid, eventually to atmospheric pressure, allowing the liquid to boil. Therefore, at the boiling point, the temperature of the pot will be higher than the temperature of the head.
Explanation:
when temperatures increase, pressures also do so, thus reaching boiling points where liquid states become gaseous.
Answer:
1.428mol of CO2
Explanation:
C2H4 + 3O2 —> 2CO2 + 2H2O
First let us calculate the number of mole present in 20g of C2H4. This is illustrated below:
Molar Mass of C2H4 = (12x2) +(1x4) = 24 + 4 = 28g/mol
Mass of C2H4 = 20g
Number of mole of C2H4 = Mass /Molar Mass
Number of mole of C2H4 = 20/28 = 0.714mol
From the balanced equation,
1mole of C2H4 produced 2moles of CO2.
Therefore, 0.714mol of C2H4 will produce = 0.714 x 2 = 1.428mol of CO2