Methanol (CH3OH) can be synthesized from carbon monoxide and hydrogen by the following reversible reaction. CO + H₂ CH3OH + energy If the temperature in the reaction chamber is increased, what happens to the yield of methanol? O increases O decreases stays the same cannot be determined If the pressure in the reaction chamber is increased, what happens to the yield of methanol? O increases O decreases O stays the same O cannot be determined

Record your two digit answer. Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI,(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer Under these conditions, the equilibrium system in Question 20 favours the forward the reverse neither reaction. ?

Are chemical reactions reversible? In other words, is it possible the reverse the direction of a reaction to convert the reaction products back into reactants?

In a reversible reaction, dynamic equilibrium is attained when which of the following occurs? The concentration of the reactants reaches zero. The concentration of the products remains constant . The rate of the reverse reaction is greater than the rate of the forward reaction. The rate of the forward reaction is greater than the rate of the reverse reaction.

The reaction diagram shown below represents an exothermic reaction. Reactants Energy released Products Direction of reaction O True False Stored chemical energy

The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g)   ⇋   4 NO (g) + 6 H2O (g) If the temperature is decrease, what happens to the concentration of H2O?

For any reversible reaction containing a double arrow such as: Reactants ⟷⟷ Products the statement "equilibrium shifts to the right" means: Group of answer choices; - The reaction can only go in the forward direction. - The reaction can only go in the reverse direction. - A stress will cause a portion of reactants to disappear and some additional products to appear. - A stress will cause a portion of products to disappear and some additional reactants to appear

What is the effect of adding a catalyst on a reaction? O It changes the equilibrium position It makes the reactants more stable O It makes the products more stable O It increases the rate OIt decreases the entropy

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Which way would the equilibrium shift if the temperature was decreased for this reaction (AH = -542 kJ)? H₂ (g) + F₂ (g) → 2HF (g) Shift toward reactants Shift toward products Remain the same None of the above