Calculate the amount of heat transferred when 24.0g of ch3oh(g) is decomposed by this reaction at constant pressure. for a given sample of ch3oh , the enthalpy change during the reaction is 82.6kj . what mass of methane gas is produced? how many kilojoules of heat are released when 38.7g of ch4(g) reacts completely with o2(g) to form ch3oh(g) at constant pressure?

94,4 kJ of heat transferred.

10,5 g of CH₄ gas are produced.

304 kJ are released.

Explanation:

The reaction is:

2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252 kJ

24,0 g of CH₃OH(g) are:

24,0g CH₃OH× = 0,749 moles of CH₃OH(g)

As two moles of CH₃OH(g) transferred +252 kJ, 0,749 moles of CH₃OH(g) transferred:

0,749 molesCH₃OH× = 94,4 kJ

When 2 moles of CH₄ are produced, the enthalpy change is +252 kJ. 82,6 kJ are:

82,6kJ×= 0,656 moles of CH₄

0,656 moles of CH₄ are:

0,656 moles of CH₄× = 10,5 g of CH₄

38,7 g of CH₄(g) are:

38,7g CH× = 2,41 moles of CH₄(g)

As two moles of CH₄ released 252 kJ, 2,41 moles of CH₄(g) released:

2,41 moles CH₄× = 304 kJ

I hope it helps!

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.