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3 years ago

How many grams of mgo are produced during an enthalpy change of -233 kj ?

1 answer:

6 0

Chemical reaction: 2Mg + O₂ → 2MgO. ΔH = -1204 kJ.
ΔH(reaction) = -233 kJ.
From chemical reaction we can se that two moles of magnesium oxide produce -1204 kJ, make proportion:
2 mol : -1204 kJ = n(MgO) : -233 kJ.
n(MgO) = 0,387 mol.
m(MgO) = n(MgO) · M(MgO).
m(MgO) = 0,387 mol · 40,3 g/mol.
m(MgO) = 15,596 g.

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How many grams of P4O10 (292.88 g/mol) form when phelpsphorous (P4, 125.52 g/mol) reacts with 16.2 L of O2 (33.472 g/mol) ) at s

nevsk [136]

Answer:

40.5 g of P₄O₁₀ are produced

Explanation:

We state the reaction:

P₄ + 5O₂ → P₄O₁₀

We do not have data from P₄ so we assume, it's the excess reactant.

We need to determine mass of oxygen and we only have volumne so we need to apply density.

Density = mass / volume, so Mass = density . volume

Denstiy of oxygen at STP is: 1.429 g/L

1.429 g/L . 16.2L = 23.15 g

We determine the moles: 23.15 g . 1mol / 33.472g = 0.692 moles

5 moles of O₂ can produce 1 mol of P₄O₁₀

Our 0.692 moles may produce (0.692 . 1)/ 5 = 0.138 moles

We determine the mass of product:

0.138 mol . 292.88 g/mol = 40.5 g

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3 years ago

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4 years ago

2ca(s)+o2(g) → 2cao(s) δh∘rxn= -1269.8 kj; δs∘rxn= -364.6 j/k

Alinara [238K]

Gibbs free energy change for the reaction at 29°C. is equal to -1378.93 KJ.

<h3>What is Gibbs's free energy?</h3>

Gibbs free energy can be described as the enthalpy of the system minus the product of the temperature and entropy.

If the chemical reaction can be carried out under constant temperature ΔT = 0:

ΔG = ΔH – TΔS

The above equation is known as the Gibbs-Helmholtz equation.

ΔG > 0 non-spontaneous and endergonic and ΔG < 0 spontaneous and exergonic, ΔG = 0 is representing equilibrium.

Given the ΔS = -364 J/K, ΔH = -1269.8 KJ, T = 29°C = 29 + 273 = 302 K

ΔG = - 1269 - 302 × 364

ΔG = -1269 KJ - 109.93 KJ

ΔG = - 1378.93 KJ

Learn more about Gibbs's free energy, here:

brainly.com/question/13318988

#SPJ1

Your question is incomplete, most probably the complete question was,

2Ca(s)+O₂(g) → 2CaO(s)

ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K

For this problem, assume that all reactants and products are in their standard states.

Calculate the free energy change for the reaction at 29°C.

6 0

2 years ago