ΔS is negative and ΔG is negative at low temperatures...
ΔS is positive and G is negative at all temp.Which of the following is true for the gas phase reaction shown below? 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g), ΔH = -2511 kJΔS is negative and ΔG is negative at low temperatures.
The equilibrium constant (Kc) for the reaction would be [O2]/([H2O2]^[H2O]) = 0.25/(0.15*0.21) = 7.94
The equilibrium constant (Kc) for a reaction can be calculated using the concentrations of the products and reactants at equilibrium. In this case, Kc = [O2]/([H2O]^2). Plugging in the given values, Kc = (0.92)/((0.37)^2) ≈ 6.56.
The reaction is exothermic because the enthalpy change (ΔH) is negative (-0.905 kJ). This means heat is released during the reaction. The reaction forms nitrogen monoxide (NO) and water (H2O) from ammonia (NH3) and oxygen (O2) in the gas phase.
The conjugate acid of HSO4- in the reaction below would be H2SO4. The conjugate acid is formed by adding a proton to the base.
ΔS is positive and G is negative at all temp.Which of the following is true for the gas phase reaction shown below? 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g), ΔH = -2511 kJΔS is negative and ΔG is negative at low temperatures.
0.34
0.28
ΔS is positive and ΔG is negative at low temperatures only
The equilibrium constant (Kc) for the reaction would be [O2]/([H2O2]^[H2O]) = 0.25/(0.15*0.21) = 7.94
H2(g) + I2(g) 2HI(g)18.6
s is positive and g i s negative at all temperatures
The equilibrium constant (Kc) for a reaction can be calculated using the concentrations of the products and reactants at equilibrium. In this case, Kc = [O2]/([H2O]^2). Plugging in the given values, Kc = (0.92)/((0.37)^2) ≈ 6.56.
Nick Bobo sucks dick
The reaction is exothermic because the enthalpy change (ΔH) is negative (-0.905 kJ). This means heat is released during the reaction. The reaction forms nitrogen monoxide (NO) and water (H2O) from ammonia (NH3) and oxygen (O2) in the gas phase.
it starts to weather (erode). Details of the chemical reaction can be found by following the link below.
I am sorry but the question is incomplete. You have not mentioned the ordered pairs and the equation is incomplete as well.