The equilibrium constant (K) of the reaction below is K = 6.0 x 102, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B IU E T O Word(s) T II

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Answer 3 please
Use this information to answer Questions 3, 4, and 5:
The equilibrium constant (K) of the reaction below is K = 6.0 x 10´2, with initial concentrations as follows:
[H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M.
N2(g) + 3H2(g) = 2NH3(g)
3. Consider the chemical reaction: N2+ 3H2yields 2NH3. If the concentration of the reactant H2 was increased from
1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would
shift by comparing the value of Q to K.
B IU E E T
T
O Word(s)
4. If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
B
T'
T
O Word(s)
5. If the concentration of the product NH3 was increased from 1.0x 104M to 5.6 x 103 M, calculate the reaction
quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
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Transcribed Image Text:Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10´2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10 M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2+ 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0x 102 M to 2.5x 101 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B IU E E T T O Word(s) 4. If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B T' T O Word(s) 5. If the concentration of the product NH3 was increased from 1.0x 104M to 5.6 x 103 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. O Word(s) 80 888 DII FB F11 23 & 2 3 4 5 6 7 8 9 - W E R Y U { P D G H J K с V N > mmand command option .. .- - ※口
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