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Please help.. . At a certain temperature, 0.3811 mol of N2 and 1.641 mol of H,...
Question 10 of 23 > At a certain temperature, 0.4011 mol of N2 and 1.641 mol of H2 are placed in a 4.00 L container N2(g)+3 H2 g) 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Ke
At a certain temperature, 0.4811 mol of N2 and 1.801 mol of H2 are placed in a 2.50 L container. N2(g)+3H2(g)−⇀↽−2NH3(g) At equilibrium, 0.1001 mol of N2 is present. Calculate the equilibrium constant, Kc. Kc=
At a certain temperature, 0.3611 mol of N, and 1.641 mol of H, are placed in a 3.00 L container. N_(8) + 3H,() 2NH,(6) At equilibrium, 0.1201 mol of N, is present. Calculate the equilibrium constant, Ke. At a certain temperature, 0.3611 mol of N, and 1.641 mol of H, are placed in a 3.00 L container. Ny()+ 3H2(g) + 2NH,(g) At equilibrium, 0.1201 mol of N, is present. Calculate the equilibrium constant, K. K =
1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a 4.00 L container. CH4(g)+2H2O(g)????CO2(g)+4H2(g) At equilibrium, 4.89 g CO2 is present. Calculate Kc. 2. At a certain temperature, 0.352 mol CH4 and 0.862 mol H2S are placed in a 1.50 L container. CH4(g)+2H2S(g)????CS2(g)+4H2(g) At equilibrium, 14.5 g CS2 is present. Calculate Kc . 3. At a certain temperature, 0.3211 mol of N2 and 1.501 mol of H2 are placed in a 2.50 L container....
At a certain temperature, 0.4011 mol of N, and 1.541 mol of H, are placed in a 2.00 L container. N2(g) + 3H2(g) = 2 NH3(g) At equilibrium, 0.1201 mol of N, is present. Calculate the equilibrium constant, Kc. Kc =
At a certain temperature, 0.4411 mol of N2 and 1.581 mol of H2 are placed in a 1.50 L container.N2(g)+3H2(g)⇌2NH3(g)At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.Kc=_____
At a certain temperature, 0.4411 mol of N2 and 1.521 mol of H2 are placed in a 3.00 L container. N2(g)+3H2(g)−⇀↽−2NH3(g) At equilibrium, 0.1601 mol of N2 is present. Calculate the equilibrium constant, Kc.
At a certain temperature, 0.4011 mol of N2 and 1.721 mol of H2 are placed in a 4.50 L container. N2(g)+3H2(g)↽−−⇀2NH3(g) N 2 ( g ) + 3 H 2 ( g ) ↽ − − ⇀ 2 NH 3 ( g ) At equilibrium, 0.1601 0.1601 mol of N2 N 2 is present. Calculate the equilibrium constant, ?c K c .
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
At a certain temperature, 0.760 mol SO3is placed in a 2.50 L container.2SO3(g)⇌2SO2(g)+O2(g)At equilibrium, 0.130 mol O20.130 mol O2 is present. Calculate Kc.