2NOBr(g)(double arrow)2NO(g) + Br2(g) If 0.382 moles of NOBr(g), 0.517 moles of NO, and 0.579 moles...
2NOBr(g)(double
arrow)2NO(g) +
Br2(g)
If 0.382 moles of NOBr(g),
0.517 moles of NO, and
0.579 moles of Br2 are
at equilibrium in a 17.5L container at
522 K, the value of the equilibrium constant,
Kc, is
Homework Answers
![2 NOBr Kc= - 2NO+ Brz. [N01² [Brz]? No Br72 6.579 17.5 0 382)2 178 - (0:517)*(0.579) (1715) (0.382)2 = 0.0606. And.](http://img.homeworklib.com/questions/630b0d70-da7f-11eb-90dd-91c21979472f.png?x-oss-process=image/resize,w_560)
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2NOBr(g)(double
arrow)2NO(g) +
Br2(g)
If 0.382 moles of NOBr(g),
0.517 moles of NO, and
0.579 moles...
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g)...
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g) When she introduced 0.185 moles of NO(g) and 0.130 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.152 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 295 K: 2NO(g) + Br2(g) <--->...
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When
she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into
a 1.00 liter container, she found the equilibrium concentration of
NOBr(g) to be 0.107 M.
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The square in the reaction equation is an equilibrium sign. Consider the following reaction: 2NOBr(g) 2NO(g)...
The square in the reaction equation is an equilibrium
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Consider the following reaction where Kc = 154 at 298 K: 2NO(g) + Br2(g) 2NOBr(g) A...
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A student ran the following reaction in the laboratory at 225 K: 2NOBr(g) 2 2NO(g) +...
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Consider the following reaction where Kc = 154 at 298 K. 2NO(g) + Br2(g) 2NOBr(g) A...
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When
she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into
a 1.00 liter container, she found the equilibrium concentration of
NOBr(g) to be 0.107 M.
A student ran the following reaction in the laboratory at 297 K: 2NO(g)+ Br2(g)2NOBr(g) When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M. Calculate the equilibrium constant, Kc, she obtained for this reaction....
The square in the reaction equation is an equilibrium
sign.
Consider the following reaction: 2NOBr(g) 2NO(g) + Br2(g) If 0.485 moles of NOBr(g), 0.623 moles of NO, and 0.470 moles of Br2 are at equilibrium in a 14.9 L container at 494 K, the value of the equilibrium constant, Kc, is The equilibrium constant, K. , for the following reaction is 7.00x10- at 673 K. NHI(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.01...
A student ran the following reaction in the laboratory at 225 K: 2NOBr(g) 2 2NO(g) + Brz(g) When she introduced 0.198 moles of NOBr(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 1.89x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g) A reaction mixture was found to contain 2.86x10-2 moles of NO(g), 3.93x10-2 moles of Br2(g) and 8.83x10-2 moles of NOBr(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed. 2. In order to reach equilibrium K, must increase. 3. In order to reach equilibrium NO must be...
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