The new temperature : 11.56 °C
<h3>Further explanation </h3>
Boyle's law and Gay Lussac's law

P1 = initial gas pressure (N/m² or Pa)
V1 = initial gas volume (m³)
P2 = final gas pressure
V2 = final gas volume
T1 = initial gas temperature (K)
T2 = final gas temperature
V₁=4.39 L
T₁=44+273=317 K
P₁ = 729 torr = 0,959211 atm
V₂=3.78 L
P₂= 1 atm

Answer: The molar enthalpy change is 73.04 kJ/mol
Explanation:

moles of HCl= 
As NaOH is in excess 0.0415 moles of HCl reacts with 0.0415 moles of NaOH.
volume of water = 100.0 ml + 50.0 ml = 150.0 ml
density of water = 1.0 g/ml
mass of water = 

q = heat released
m = mass = 150.0 g
c = specific heat = 
= change in temperature = 


Thus 0.0415 mol of HCl produces heat = 3031.3 J
1 mol of HCL produces heat = 
Thus molar enthalpy change is 73.04 kJ/mol
Answer:
i think the answer is C , atom mass increases with temperature
Answer:
ΔH°_rxn = -195.9 kJ·mol⁻¹
Explanation:
4NH₃(g) + 3O₂(g) ⟶ 2N₂(g) +6H₂O(g)
ΔH°_f/(kJ·mol⁻¹): -45.9 0 0 -241.8
The formula relating ΔH°_rxn and enthalpies of formation (ΔH°_f) is
ΔH°_rxn = ΣΔH°_f(products) – ΣΔH°_f(reactants)
ΣΔH°_f(products) = -6(241.8) = -1450.8 kJ
ΣΔH°_f(reactants) = -4(45.9) = -183.6 kJ
ΔH°_rxn = (-1450.8 + 183.6) kJ = -1267.2 kJ