To calculate the amount of heat transferred when an amount of reactant is decomposed, we must look at the balanced reaction and its corresponding heat of reaction. In this case, we can see that 252.8 kJ of heat is transferred per 2 moles of CH3OH used. When 22 g of CH3OH is used, 86.9 kJ is absorbed.
Answer:
moles of CO2 can be produced from a reaction of 10.0 moles C2H6
Explanation:
In this reaction -
2 moles of C₂H6 produces four molecules of Carbon dioxide (CO2)
So 1 mole of C₂H6 will produce 
moles of Carbon dioxide (CO2)
Thus, 10 moles of C₂H6 will produce 
moles of Carbon dioxide (CO2)
Atomic number equals the number of protons or electrons. Atomic mass equals the number of protons and neutrons
For a neutral solution,
[H+][OH-] = 1 x 10⁻¹⁴
Answer:
0.595
Explanation:
Let's consider the decomposition of hydrogen chloride.
2 HCl(g) ⇄ H₂(g) + Cl₂(g)
The pressure equilibrium constant (Kp) is equal to the product of the partial pressure of the products raised to their stoichiometric coefficients divided by the product of the partial pressure of the reactants raised to their stoichiometric coefficients.
Kp = pH₂ × pCl₂ / pHCl²
Kp = 77.9 × 54.4 / 84.4²
Kp = 0.595
