Chemistry, 14.05.2021 21:30 Artemis3821
Consider the following reation: 2NO(g) + 2H2(g) = N2(g) + 2H208)
Starting concentrations of 0.10M NO, 0.050M H2 and 0.10M water vapor are placed in a reaction vessel. The system then establishes
equilibrium. At equilibrium (NO) = 0.062M. Complete the following ICE Chart.
Answers: 2
Chemistry, 22.06.2019 04:50
Compare the equilibrium constants for the systems shown in the table. which favors products the most? which favors products the least? rank these systems in order from most to least in terms of favoring products rather than reactants. d > b > a > c c > a > b > d b > c > d > a a > d > c > b
Answers: 1
Chemistry, 22.06.2019 14:30
For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants. 4al(s)+3o2(g)→2al2o3(s) a) 1 molal, 1 mol o2 b) 4 molal, 2.6 mol o2 c) 16 molal, 13 mol o2 d) 7.4 molal, 6.5 mol o2
Answers: 3
Chemistry, 22.06.2019 21:00
The rate constant for the reaction below is 6.2 x 10−5 mol l−1 s −1. if the initial concentration of a is 0.0500 m, what is its concentration after 115 s?
Answers: 1
Consider the following reation: 2NO(g) + 2H2(g) = N2(g) + 2H208)
Starting concentrations of 0.10M N...
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