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化學英文計算
1.Urea, (NH2)2CO, can be prepared by heating ammonium cyanate, NH40CN. NH4OCN變成(NH2)2COThis reaction may occur by the following mechanism: NH4+ + OCN變成( NH) +HOCN fast eqllilibriumNH3 + HOCN 變成( NH2)2CO slowWhat is the rate law predicted by this mechanis2. When calciwn carbonate, CaCO), is... 顯示更多 1. Urea, (NH2)2CO, can be prepared by heating ammonium cyanate, NH40CN. NH4OCN變成(NH2)2CO This reaction may occur by the following mechanism: NH4+ + OCN變成( NH) +HOCN fast eqllilibrium NH3 + HOCN 變成( NH2)2CO slow What is the rate law predicted by this mechanis 2. When calciwn carbonate, CaCO), is heated, it decomposes to calcium oxide. CaC03(s)→ CaO(s)+CO2(g);＊熱H=178.3kJ. How much heat is required to decompose 10 g of calcium carbonate? (atornic weight: Ca = 40, C = 12, 0 = 16) 3.A water-soluble compound of gold and chlorine is treated with silver nitrate, AgN03, to convert the chlorine completely to silver chloride, AgCl. In an experiment, 328 mg of the compound gave 464 mg of silver chloride. Calculate the percentage of Cl in the compound. What is its empirical formula? (atomic weight: Cl = 35.5, N = 14, Ag = 108, Au = 197, O=16). 請各位高手幫忙解題～ 對於化學一竅不通 謝謝～ 更新: 謝謝賣女孩的火才
最佳解答:
1. The reaction : NH4OCN → (NH2)2CO Mechanism : Step 1 : NH4? + OCN? ? NH3 + HOCN (equilibrium constant = Ka)(fast) Step 2 : NH3 + HOCN → (NH2)2CO (slow) From step 1 : Ka = [NH3] [HOCN] / [NH4?] [OCN?] Hence, [NH3] [HOCN] = Ka [NH4?] [OCN?] ...... (1) From step 2 : Rate = k' [NH3] [HOCN] ...... (2) Substitute (1) into (2) : Rate = k' Ka [NH4?] [OCN?] Hence, Rate = k [NH4?] [OCN?] 2. CaCO3(s) → CaO(s) + CO2(g) .. ΔH = +178.3 kJ When 1 mol of CaCO3 is decomposed, 178.3 kJ of heat is required. No. of moles of CaCO3 = 10/(40 + 12 + 16x3) = 0.1 mol Amount of heat required = 178.3 x 0.1 = 17.83kJ 3. Mass fraction of Cl in AgCl = 35.5/(108 + 35.5) = 35.5/143.5 Mass of Cl in 464 g of AgCl = 464 x (35.5/143.5) = 114.8 mg In 328 mg of the compound : Mass of Cl = 114.8 mg Mass of Au = 328 - 114.8 = 213.2 mg In the compound, mole ratio Au : Cl = 213.2/197 : 114.8/35.5 = 1.08 : 3.23 ≈ 1 : 3 Hence, empirical formula = AuCl3
其他解答:5C926699F268FE02
化學英文計算
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發問:1.Urea, (NH2)2CO, can be prepared by heating ammonium cyanate, NH40CN. NH4OCN變成(NH2)2COThis reaction may occur by the following mechanism: NH4+ + OCN變成( NH) +HOCN fast eqllilibriumNH3 + HOCN 變成( NH2)2CO slowWhat is the rate law predicted by this mechanis2. When calciwn carbonate, CaCO), is... 顯示更多 1. Urea, (NH2)2CO, can be prepared by heating ammonium cyanate, NH40CN. NH4OCN變成(NH2)2CO This reaction may occur by the following mechanism: NH4+ + OCN變成( NH) +HOCN fast eqllilibrium NH3 + HOCN 變成( NH2)2CO slow What is the rate law predicted by this mechanis 2. When calciwn carbonate, CaCO), is heated, it decomposes to calcium oxide. CaC03(s)→ CaO(s)+CO2(g);＊熱H=178.3kJ. How much heat is required to decompose 10 g of calcium carbonate? (atornic weight: Ca = 40, C = 12, 0 = 16) 3.A water-soluble compound of gold and chlorine is treated with silver nitrate, AgN03, to convert the chlorine completely to silver chloride, AgCl. In an experiment, 328 mg of the compound gave 464 mg of silver chloride. Calculate the percentage of Cl in the compound. What is its empirical formula? (atomic weight: Cl = 35.5, N = 14, Ag = 108, Au = 197, O=16). 請各位高手幫忙解題～ 對於化學一竅不通 謝謝～ 更新: 謝謝賣女孩的火才
最佳解答:
1. The reaction : NH4OCN → (NH2)2CO Mechanism : Step 1 : NH4? + OCN? ? NH3 + HOCN (equilibrium constant = Ka)(fast) Step 2 : NH3 + HOCN → (NH2)2CO (slow) From step 1 : Ka = [NH3] [HOCN] / [NH4?] [OCN?] Hence, [NH3] [HOCN] = Ka [NH4?] [OCN?] ...... (1) From step 2 : Rate = k' [NH3] [HOCN] ...... (2) Substitute (1) into (2) : Rate = k' Ka [NH4?] [OCN?] Hence, Rate = k [NH4?] [OCN?] 2. CaCO3(s) → CaO(s) + CO2(g) .. ΔH = +178.3 kJ When 1 mol of CaCO3 is decomposed, 178.3 kJ of heat is required. No. of moles of CaCO3 = 10/(40 + 12 + 16x3) = 0.1 mol Amount of heat required = 178.3 x 0.1 = 17.83kJ 3. Mass fraction of Cl in AgCl = 35.5/(108 + 35.5) = 35.5/143.5 Mass of Cl in 464 g of AgCl = 464 x (35.5/143.5) = 114.8 mg In 328 mg of the compound : Mass of Cl = 114.8 mg Mass of Au = 328 - 114.8 = 213.2 mg In the compound, mole ratio Au : Cl = 213.2/197 : 114.8/35.5 = 1.08 : 3.23 ≈ 1 : 3 Hence, empirical formula = AuCl3
其他解答:5C926699F268FE02
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