For the chemical equation
SO2(g) + NO2(g) – SO2(g) + NO(g)
the equilibrium constant at a certain temperature is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.31 mol SO2(g) in order to form 1.10 mol SO3(g) at equilibrium.
moles of NO2(g): _______ mol
For the chemical equation SO2(g) + NO2(g) – SO2(g) + NO(g) the equilibrium constant at a...
At a certain temperature, the equilibrium constant for the following chemical equation is 3.30. SO2(g) + NO2(g) <---> SO3(g) + NO(g), At this temp, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.
For the chemical equation SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.20 mol SO2(g) in order to form 1.00 mol SO3(g) at equilibrium. moles of NO2(g):
For the chemical equation SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) the equilibrium constant at a certain temperature is 2.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 3.36 mol SO2(g) in order to form 1.40 mol SO3(g) at equilibrium.
For the chemical equation SO2(g) + NO2(g) → SO2(g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.99 mol SO,(g) in order to form 1.30 mol S03(g) at equilibrium. moles of NO2(g): mol
For the chemical equationSO2(g)+NO2(g) SO3(g)+NO(g)SO2(g)+NO2(g) SO3(g)+NO(g)the equilibrium constant at a certain temperature is 2.40.2.40. At this temperature, calculate the number of moles of NO2(g)NO2(g) that must be added to 2.75 mol SO2(g)2.75 mol SO2(g) in order to form 1.10 mol SO3(g)1.10 mol SO3(g) at equilibrium.moles of NO2(g):NO2(g):
For the chemical equation SO2(g) + NO (g) = 30,(g) + NO(g) the equilibrium constant at a certain temperature is 3.30. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.76 mol SO2(g) in order to form 1.20 mol SOz (g) at equilibrium.
a certain temperature, the equilibrium constant for the following chemical equation is 2.50. SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.76 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium. Number _______ mol of NO2(g)
For the chemical equation S0,(g) + NO,(g) SO,()+NO(g) the equilibrium constant at a certain temperature is 2.80. At this temperature, calculate the number of moles of NO,(g) that must be added to 3.08 moles of SO,(g) in order to form 1.40 moles of SO,(g) at equilibrium. mol mo
I'll rate first right answer. The equilibrium constant for the reaction SO2(g)+NO2(g)⇌SO3(g)+NO(g) is 3.1. Find the amount of NO2 that must be added to 2.6 mol of SO2 in order to form 1.1 mol of SO3 at equilibrium.
At some temperature, the value of the equilibrium constant for the reaction: SO2 (g) + NO2(g) ↔ SO3(g) + NO(g) has the value K = 0.640. If all four gases are placed into a container, each with an initial partial pressure of 1.25 atm, calculate the equilibriuym partial pressure (in atm) of SO3(g)