At 10 k cp, m(hg(s)) = 4.64 j k−1 mol−1. between 10 k and the melting point of hg(s), 234.3 k, heat capacity measurements indicate that the entropy increases by 57.74 j k−1 mol−1. the standard enthalpy of fusion of hg(s) is 2322 j mol−1 at 234.3 k. between the melting point and 298.0 k, heat capacity measurements indicate that the entropy increases by 6.85 j k−1 mol−1. determine the third-law standard molar entropy of hg(l) at 298 k.
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Chemistry, 22.06.2019 17:00, abbygailgo674
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Answer asap need it by wednesday morning carry out the following calculations on ph and ka of from data. i. calculate the ph of 0.02m hcl ii. calculate the ph of 0.036m naoh iii. calculate the ph of 0.36m ca(oh)2 iv. calculate the ph of 0.16m ch3cooh which has ka = 1.74 x 10-5 mol dm-3 v. calculate ka for weak acid ha which has a ph of 3.65 at 0.30m concentration vi. calculate the ka of a solution made by mixing 15.0 cm3 0.2m ha and 60.0 cm3 0.31m a-. [ph= 3.80] vii. calculate the ph of a solution made by mixing 15.0 cm3 0.1m naoh and 35.0 cm3 0.2m hcooh. [ka = 1.82 x 10-4 m]
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Chemistry, 23.06.2019 00:30, hdhshshs741
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At 10 k cp, m(hg(s)) = 4.64 j k−1 mol−1. between 10 k and the melting point of hg(s), 234.3 k, heat...
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