Chemistry, 22.09.2019 10:00 colton6926
You need to make a stock solution of a known copper concentration for your experiment. you start by weighing out a piece of pure copper wire which has a mass of 0.211 g. you then add 1.0 ml of 12 m hno3, 3.0 ml of h2o and 2.0 ml of 12 m nh4oh to dissolve the copper metal.
the moles of copper that are in the solution = 0.00332 mols. now i need to find the final molarity of copper in the solution.
Answers: 1
Chemistry, 21.06.2019 18:30
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Be sure to answer all parts. the following equilibrium constants were determined at 1123 k: c(s) + co2(g) ⇌ 2co(g) k'p = 1.30 × 1014 co(g) + cl2(g) ⇌ cocl2(g) k''p = 6.00 × 10−3 calculate the equilibrium constant at 1123 k for the reaction: c(s) + co2(g) + 2cl2(g) ⇌ 2cocl2(g) 4.68 × 10 9 (enter your answer in scientific notation.) write the equilibrium constant expression, kp:
Answers: 3
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