When methanol, ch 3 oh , is burned in the presence of oxygen gas, o 2 , a large amount of heat energy is released. for this reason, it is often used as a fuel in high performance racing cars. the combustion of methanol has the balanced, thermochemical equation

ch3oh(g)+3/2o2(g) ⟶ co2(g) + 2h2o(i) δ h = − 764 kj.

how much methanol, in grams, must be burned to produce 575 kj of heat?

24.1 g

Explanation:

Let's consider the following thermochemical equation.

CH₃OH(g) + 3/2 O₂(g) ⟶ CO₂(g) + 2 H₂O(I) ΔH = − 764 kJ

In order to produce 764 kJ of heat, 1 mole of methanol must be burned. To produce 575 kJ, the required moles of methanol are:

-575 kJ × (1 mol CH₃OH/ -764 kJ) = 0.753 mol CH₃OH

The molar mass of methanol is 32.04 g/mol. 0.753 moles of methanol represent a mass of:

mass = moles × molar mass

0.753 mol × (32.04 g/mol) = 24.1 g

b i think it’s a water wheel turning in a stream

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa