The lowest point of a wave is called trough.
Answer:
2.53 grams of hydrogen gas will be produced and 12.2 many grams of the excess reactant i.e. calcium will be left over.
Explanation:
Moles of calcium = 
Moles of HCl = 
According to reaction, 2 moles of HCl reacts with 1 mole of calcium :
Then 2.53 moles of HCl will recat with :
of calcium.
As we can see moles of calcium are in excessive amount. Hence calcium is an excessive reagent.
Moles of calcium left unreacted =1.57 mol - 1.265 mol =0.305 mol
Mass calcium left unreacted = 0.305 mol × 40 g/mol =12.2 g
Since, calcium is an excessive reagent HCl is limiting reagent and the amount of hydrogen gas produced will depend on HCl .
According to reaction, 2 moles of HCl gives 1 mole of hydrogen gas.
Then 2.53 moles of HCl will give:
of hydrogen gas.
Mass of 1.265 mol of hydrogen gas = 1.265 mol × 2 g/mol = 2.53 g
2.53 grams of hydrogen gas will be produced and 12.2 many grams of the excess reactant i.e. calcium will be left over.
Answer:
The chlorine gas and potassium bromide solution react to form liquid bromine and potassium chloride solution.
Explanation:
Chemical equation:
Cl₂(g) + KBr (aq) → KCl (aq) + Br₂(l)
Balanced chemical equation:
Cl₂(g) + 2KBr (aq) → 2KCl (aq) + Br₂(l)
This equation showed that the chlorine gas and potassium bromide solution react to form liquid bromine and potassium chloride solution.
Chlorine is more reactive than bromine it displace the bromine from potassium and form potassium chloride solution.
The given equation is balanced and completely hold the law of conservation of mass.
According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.
Explanation:
This law was given by french chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.
Starch Im pretty sure correct me if Im wrong Hope I helped
Answer:
ΔH of CH4(g)+2O2(g)→CO2(g)+2H2O(l) is -899 KJ
Explanation:
step 1: write down thye reaction and rearrange them in a way that similar contents cancel out to produce the required reaction and add the enthalpy change of each.
CH4(g)+O2(g)→CH2O(g)+H2O(g) ΔH = -284 KJ
CH2O(g)+O2(g)→CO2(g)+H2O(g) ΔH = -527 KJ
2H2O(g)→2H2O(l) ΔH = 44 KJ x -2
the minus is because the last reaction has been reversed and multiplied by 2 so that the gaseous state H2O cancels with the others to leave liquid H2O in the required final reaction.
ΔHrxn = (-284)+(-527)+[44 x (-2)] = -899 KJ
