In the reaction below N2(g)+3H2(g)⇔ 2NH3(g)  deltaH = -92kJ Which of the following changes will increase the amount of ammonia at equilibrium? 1. Decreasing the temperature 2. Increassing the temperature 3. Adding a catalyst

An industrial chemist puts 1.00 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.65 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g)

Consider this system at equilibrium. A(aq) = B(aq) AH = -650 kJ/mol What can be said about Q and K immediately after an increase in temperature? O Q > K because K decreased. Q K because Q increased. How will the system respond to a temperature increase? no change shift left shift right

Indicate how equilibrium would be shifted with the following changes to the equilibrium reaction below. N2(g) + O2(g) → 2 NO(9) AH = +180 kJ/mol decrease temperature 1. shift left Add N2(g) 2. no change decrease pressure 3. shift right Remove NO(g)

Consider the following equilibrium: N₂ (g) + 3H₂ (g) 2NH3 (g) AG=-34. KJ Now suppose a reaction vessel filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about this system: Under these conditions, will the pressure of N, tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N₂ will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N₂ will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to significant digits. Ⓒrise fall O yes O no atm X S ? do Är

An industrial chemist puts 1.05 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.77 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g)

101edu.co b For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.230 atm. What is AG for this reaction? (R = 8.314 J/mol-K). 1 Q 2 W 3 E $ 4 R % 5 T Question 12 of 12 A 6 & 7 Presen 8 Home ( 9 End C

The equilibrium reaction Fez O4(s) + 3 H2(g) 2 3 Fe(s) +4 H20(g) has AH° = 149.77 kJ/mol. Write down Shift Left, Shift Right, or No Change for each of the following situations: a) Solid Fe is added to the reaction. b) The temperature of the reaction is increased. c) The volume of the reaction vessel is suddenly doubled with no change in temperature. d) After doubling the volume of the reaction vessel, the partial pressure of H20 is tripled with no change in temperature.

Consider the reaction below at equilibrium:   A (g) + 2 B (g) <-> 3 C (g)  ΔH = -234.8 kJ   Explain three ways in which the reaction can "shift to the right".  Hint: What will happen if more reactant or product is added?

Consider the following equilibrium: N₂O₂ (g) 2NO₂ (g) 2 AG=5.4 kJ Now suppose a reaction vessel is filled with 2.57 atm of dinitrogen tetroxide (N₂O4) at 138. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. rise fall O yes no 10 FAED alo Ar