Given the reaction 3C(s) + 4H2(g) + 5O2(g) ---> 3CO2(g) + 4H2O(l) ÄH= -2323.7 kJ
How much heat would be released when 34.1 g of H2 react?
2323.7 kJ x (34.1/8)) = ??
9904.7 is the answer but I already tried that and its not working
it worked now, thank you!
To find out how much heat is released when a given amount of H2 reacts, we need to use the stoichiometry of the reaction and the given enthalpy change (ÄH) value.
First, we need to determine the molar mass of H2. Hydrogen (H) has a molar mass of approximately 1 g/mol, so the molar mass of H2 is 2 g/mol.
Next, we convert the given mass of H2 (34.1 g) to moles. To do this, we divide the mass by the molar mass:
34.1 g H2 / 2 g/mol H2 = 17.05 mol H2
Now, we can use the balanced equation to determine the mole ratio between H2 and ÄH.
According to the balanced equation, the coefficient of H2 is 4, meaning that 4 moles of H2 are required to release the given ÄH value of -2323.7 kJ.
Therefore, we can set up a proportion to find the amount of heat released when 17.05 mol H2 reacts:
4 mol H2 / -2323.7 kJ = 17.05 mol H2 / x kJ
Cross-multiplying and solving for x:
x = (17.05 mol H2 * -2323.7 kJ) / 4 mol H2 = -9857.95 kJ
So, when 34.1 g of H2 reacts, approximately -9857.95 kJ of heat is released. Note that the negative sign indicates that the reaction is exothermic, meaning it releases heat.