Amixture of cs2(g) and excess o2(g) is placed in a 10 l reaction vessel at 100.0 ∘c and a pressure of 3.15 atm . a spark causes the cs2 to ignite, burning it completely, according to the equation: cs2(g)+3o2(g)→co2(g)+2so2(g) after reaction, the temperature returns to 100.0 ∘c, and the mixture of product gases (co2, so2, and unreacted o2) is found to have a pressure of 2.50 atm . what is the partial pressure of each gas in the product mixture? enter your answers numerically separated by commas.

0.65, 1.30, 0.55

Explanation:

By the Raoult's Law, the partial pressure of a gas in a gas mixture is its molar fraction multiplied by the total pressure of the mixture. Let's found out the total number of moles of the mixture using the ideal gas law:

PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature (100°C + 273 = 373 K).

3.15*10 = n*0.082*373

30.586n = 31.5

n = 1.03 moles of the reactants

Let's call the total number of moles of CS₂ as x and the number of moles of O₂ is 1.03 - x, thus by the stoichiometry of the reaction, 1:3:1:2, the number of moles of O₂ that reacts is 3x, and the remaining number of moles of it, and the number of moles of each product is:

nO₂ = (1.03 - x) - 3x

nCO₂ = x

nSO₂ = 2x

After the reaction happened, the number of moles is:

2.50*10 = n*0.082*373

30.586n = 25.0

n = 0.8174 mol

Thus,

nO₂ + nCO₂ + nSO₂ = 0.8174

(1.03 - x) -3x +x + 2x = 0.8174

1.03 - x = 0.8174

x = 0.2126 mol

nO₂ = (1.03 - 0.2126) - 3*0.2126 = 0.1796 mol

nCO₂ = 0.2126 mol

nSO₂ = 2*0.2126 = 0.4252 mol

Using Roult's Law, the partial pressures will be:

pCO₂ = (nCO₂/n)*2.50 = (0.2126/0.8174)*2.50 = 0.65 atm

pSO₂ = (nSO₂/n)*2.50 = (0.4252/0.8174)*2.50 = 1.30 atm

pO₂ = (nO₂/n)*2.50 = (0.1796/0.8174)* 2.50 = 0.55 atm

most likely he is cheating on you

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.