Any reaction that absorbs 350 kcal of energy can be classified as __________.   2. In the following gas phase reaction, what is the effect on the direction of the reaction if more O 3 is added to the reaction mixture?  3 O 2( g) + heat    2 O 3( g The position of the equilibrium remains unchanged. The equilibrium shifts to produce more products. The equilibrium shifts to produce more reactants. The rate of formation of products is increased. The catalyst for the reaction is used up.   3. What type of compound is CH 3 -CH 2 - CH 2-I ?

Consider the following equilibrium reaction taking place inside of a closed 3.0 L container: N2(g) + 3H2(g) = 2 NH3(g) Initially there are 4.5 mol/L of nitrogen gas and 10.4 mol/L of hydrogen gas. When the system reaches equilibrium, there are 3.1 mol/L of nitrogen gas remaining. What is the final concentration of hydrogen and ammonia present in the container?

Increase in temperature where will the equilibrium shift?

Can you show me how to answer this type of question I found on a online practice organic chemistry review.

The following reaction components are at equilibrium, and the reaction is exothermic in the direction written below. Which change will shift the equilibrium in a direction that will result in increasing concentration of SO2 in the container? 2 SO2(3) + O2(g) =2 SO3(g) raising the temperature decreasing the temperature Removing SO3 from the reaction mixture O Adding O2 to the reaction mixture

Chemical equilibrium is the reaction state when the concentrations of reactants and products remain constant over time. The reaction does not stop, but it reaches a dynamic equilibrium when the rates of the forward and reverse reactions become equal. A mixture of reactants and products in the equilibrium state is called an equilibrium mixture. Let's consider a general reversible reaction where AA and BB are the reactants and CC and DD are the products: aA+bB⇌cC+dD�A+�B⇌�C+�D   The concentrations in an equilibrium mixture are related by the equilibrium equation Kc=[C]c[D]d[A]a[B]b�c=[C]c[D]d[A]a[B]b where Kc�c is the equilibrium constant.   Part A The following pictures represent the equilibrium mixtures of five different chemical reactions. All the reactions proceed according to the general balanced chemical reaction A+B⇌ABA+B⇌AB Red spheres represent AA atoms, blue spheres are BB atoms, and red-blue clusters are ABAB molecules. Rank the reactions in order of increasing…

Consider the gas-phase equilibrium system represented by the equation: 2H 20(g) 2 2H 2(g) + O 2(g) Given that the forward reaction (the conversion of "left-hand" species to "right-hand" species) is endothermic, which of the following changes will decrease the equilibrium amount of H2O? adding He gas increasing the temperature at constant pressure adding a solid phase calalyst decreasing the volume of the container (the total pressure increases) adding more oxygen

Write the equilibrium expression or the chemical equation of the following reactions and calculate its equilibrium constant.

Methane and hydrogen sulfide react to form hydrogen and carbon disulfide, like this: CH₂(g)+2H₂S(g) → 4H₂(g)+CS₂(g) Use this chemical equation to answer the questions in the table below. Suppose 165. mmol of CH4 and 330. mmol of H₂S are added to an empty flask. How much H₂ will be in the flask at equilibrium? Suppose 165. mmol of H, and 41.3 mmol of CS, are added to an empty flask. How much H₂ will be in the flask at equilibrium? None. O Some, but less than 660. mmol. O 660. mmol. O More than 660. mmol. O None. O Some, but less than 165. mmol. O165. mmol. More than 165. mmol. X S

6. Consider the following reaction: SO3(e)* 4.00 moles of SO2 and 5.00 moles O2 are present in a 2.00 L container at 100°C and are at equilibrium. Calculate the equilibrium concentration of SO3 and the number of moles SO3 present if the Keq = 1.47 x 10 3