Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:Consider the following equilibrium:
2NH; (g) – N, (g)+ 3H, (g)
AG = 34. kJ
Now suppose a reaction vessel is filled with 3.96 atm of ammonia (NH,) and 6.08 atm of nitrogen (N,) at 440. °C. Answer the following questions
about this system:
O rise
Under these conditions, will the pressure of NH, tend to rise or fall?
O fall
Is it possible to reverse this tendency by adding H,?
In other words, if you said the pressure of NH, will tend to rise, can that
yes
be changed to a tendency to fall by adding H,? Similarly, if you said the
O no
pressure of NH, will tend to fall, can that be changed to a tendency to
rise by adding H,?
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of H, needed to reverse it.
atm
Round your answer to 2 significant digits.
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- Use the information below to complete the chart about Le Chateliers principlearrow_forwardConsider the following equilibrium: 2NH, (g) – N, (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 5.02 atm of ammonia (NH,) and 9.40 atm of nitrogen (N,) at 159. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N, tend to rise or fall? fall Is it possible to reverse this tendency adding H2? In other words, if you said the pressure of N, will tend to rise, can that be yes changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of N, 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 H, needed to reverse it. atm Round your answer to 2 significant digits.arrow_forwardConsider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Śarrow_forward
- In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC. In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first. This mixture is also heated to 350 oC. After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?arrow_forward4. Toluene, C;H8(1), is an important organic solvent. It is made industrially from methylcyclohexane, C,H14(g): C,H14(g) + heat ? 2C;H8(1) + 3H2(g) State three different changes to an equilibrium mixture of these reacting gases that would shift the reaction toward greater production of toluene. State and explain each change.arrow_forwardConsider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.arrow_forward
- Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5arrow_forwardConsider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. OO U rise fall yes no atm x10 X Śarrow_forwardNitrogen 2NF3(g)->N2(g) + 3F2(g) When 3.15 mol of NF3 is placed in a 3.00-L container and allowed to come to equilibrium at 900 K, the mixture is found to contain 0.0563 mol of N2. What is the value of K, at this temperature? (R = 0.0821 L'atm-mol¹ K¹). (Hint: Solve for Kc first, then calculate Kp) 4.43 x 10-7 1.8 x 102 1.11 x 10-5 191 x 103 1.07 x 10-5arrow_forward
- The value of the equilibrium constant K, for the reaction below is 0.649 at 900°C. H, (g) + CO,(g) = = H,0(g) +CO(g)arrow_forwardConsider the following equilibrium: N₂ (g) + 3H₂(g) → 2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of nitrogen (N₂) and 4.50 atm of ammonia (NH3) at 250. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 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 2 significant digits. OO rise fall yes no atm ☐x10 X Śarrow_forward
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