Answer:
I don't know what to say . just for points
The reaction is an exothermic one because heat is released to the surroundings. An exothermic reaction is a chemical reaction where energy is being released as the reaction by light or heat. On the other hand, endothermic reaction needs energy input for the reaction to proceed.
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Answer:
The combustion of hydrogen–oxygen mixtures is used to produce very high temperatures (approximately 2500 °C) needed for certain types of welding operations. Consider the reaction to be
H2(g)+1/2O2(g)=H2O(g)
change in enthalpy is -241.8 kJ
What is the quantity of heat evolved, in kilojoules, when a 160 g mixture containing equal parts of H2 and O2 by mass is burned?
Explanation:
i hope this help sorry if it does not ok bye luv!!!
H₂SO₄ + 2NaOH = Na₂SO₄ + 2H₂O
v(NaOH)=46 ml=0.046 l
c(NaOH)=1.0 mol/l
v(H₂SO₄)=55 ml=0.055 l
n(NaOH)=v(NaOH)*c(NaOH)
n(H₂SO₄)=0.5n(NaOH)
c(H₂SO₄)=n(H₂SO₄)/v(H₂SO₄)=0.5*v(NaOH)*c(NaOH)/v(H₂SO₄)
c(H₂SO₄)=0.5*0.046*1.0/0.055=0.418 mol/l
The concentration of the H₂SO₄ is 0.418M.
