Answer:
After increasing the temperature of the system:
The reaction must: Run in the forward direction to restablish equilibrium.
Already at equilibrium. The concentration of Cl2 will: Increase.
Explanation:
The equilibrium constant, for an endothermic reaction (ΔH ° positive), increases with increasing temperature.
The principle of Le Châtelier indicates that if an equilibrium mixture is heated, and consequently its temperature increases, there will be a net reaction in the direction that counteracts the disturbance caused by the increase in temperature. For an endothermic reaction, the direct reaction absorbs energy in the form of heat.
Consequently, the equilibrium shifts to the side of the products, which means that Kc increases with increasing temperature.
35.0 g would be the mass according to law of mass conservation in an isolated system in this case closed jar
1) Excess reagent
1 mol N2 / 3 mol H2
6.0 mol N2 *3 mol H2 / 1 mol N2 = 18 mol H2
18mol H2 > 12 mol H2 => H2 is limiting (you need 18 mol H2 to use all the 6 mol N2), then N2 is in excees.
12.0 mol H2 * 1mol N2/ 3 mol H2 = 4 mol N2 is the quantity that will react, then the excess is 6 mol N2 - 4 mol N2 = 2 mol N2
2) NH3 produced
12 mol H2 * [2 mol NH3 / 3 mol H2] = 8 mol NH3
Aslso, 4 mol N2 *[2molNH3 / 1 molN2] = 8 mol NH3, the same result.
3) Yield
80% * 8 mol NH3 = 6.4 mol NH3
Answer:
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Explanation:
