Consider the following reaction where K. = 83.3 at 500 K. PCI3(g) + Cl2(g)=PC!g(g) A reaction mixture was found to contain 2.92x102 moles of PCI3(g), 3.78×102 moles of C2(g) and 0.121 moles of PClg(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
Consider the following reaction where K. = 83.3 at 500 K. PCI3(g) + Cl2(g)=PC!g(g) A reaction mixture was found to contain 2.92x102 moles of PCI3(g), 3.78×102 moles of C2(g) and 0.121 moles of PClg(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
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Chapter1: Chemical Foundations
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I dont know how to do these two question on reaction quotient
![Consider the following reaction where \( K_c = 6.50 \times 10^{-3} \) at 298 K.
\[ 2 \text{NOBr}(g) \rightleftharpoons 2 \text{NO}(g) + \text{Br}_2(g) \]
A reaction mixture was found to contain \( 9.28 \times 10^{-2} \) moles of NOBr(g), \( 2.50 \times 10^{-2} \) moles of NO(g), and \( 4.18 \times 10^{-2} \) moles of Br\(_2(g)\), in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?
The reaction quotient, \( Q_c \), equals [Text Box]
The reaction:
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.
[Submit Answer] [Retry Entire Group] 9 more group attempts remaining
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Transcribed Image Text:Consider the following reaction where \( K_c = 6.50 \times 10^{-3} \) at 298 K.
\[ 2 \text{NOBr}(g) \rightleftharpoons 2 \text{NO}(g) + \text{Br}_2(g) \]
A reaction mixture was found to contain \( 9.28 \times 10^{-2} \) moles of NOBr(g), \( 2.50 \times 10^{-2} \) moles of NO(g), and \( 4.18 \times 10^{-2} \) moles of Br\(_2(g)\), in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?
The reaction quotient, \( Q_c \), equals [Text Box]
The reaction:
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.
[Submit Answer] [Retry Entire Group] 9 more group attempts remaining
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![Consider the following reaction where \( K_c = 83.3 \) at 500 K.
\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]
A reaction mixture was found to contain \( 2.92 \times 10^{-2} \) moles of \( \text{PCl}_3(g) \), \( 3.78 \times 10^{-2} \) moles of \( \text{Cl}_2(g) \), and 0.121 moles of \( \text{PCl}_5(g) \), in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?
The reaction quotient, \( Q_c \), equals \_\_\_\_\_\_\_
The reaction:
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.
- **Submit Answer**
- **Retry Entire Group**
9 more group attempts remaining
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Transcribed Image Text:Consider the following reaction where \( K_c = 83.3 \) at 500 K.
\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]
A reaction mixture was found to contain \( 2.92 \times 10^{-2} \) moles of \( \text{PCl}_3(g) \), \( 3.78 \times 10^{-2} \) moles of \( \text{Cl}_2(g) \), and 0.121 moles of \( \text{PCl}_5(g) \), in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?
The reaction quotient, \( Q_c \), equals \_\_\_\_\_\_\_
The reaction:
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.
- **Submit Answer**
- **Retry Entire Group**
9 more group attempts remaining
**Navigation:**
- **Previous**
- **Next**
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Expert Solution
Step 1
Please note: According to the guideline, in one session only one question can be solved. Ask the second question in a separate session.
Phosphorus trichloride reacts with oxygen to form phosphorus pentachloride. The equation for the balanced chemical reaction is as follows:
The value of the equilibrium constant is = 83.3 at 500 K
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