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f.5 chem question again ~~
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最佳解答:
a. Chemical equation: Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) b.i. Average rate = Mass / time = 0.36 / 90 = 0.004 g / s ii. No. of mole of Mg in 0.004 g = Mass / molar mass = 0.004 / 24.0 = 1.67 X 10-4 mol So, average rate = no. of mole / time = 1.67 X 10-4 / 90 = 1.85 X 10-6 mol / s iii. Mole ratio of Mg to H2 = 1 : 1 So, no. of mole of H2 produced = 1.67 X 10-4 mol So, volume of H2 produced per second = 1.67 X 10-4 X 24 000 = 4 cm3 / s
其他解答:
a) Mg+2HCl>MgCl2+H2 bi)Molar mass of Mg=24.3g/mol Molar mass of HCl=1.0+35.5=36.5g/mol Number of mole of Mg=mass of Mg / molar mass of Mg =0.36 / 24.3 =0.0148mol Number of mole of HCl= molarity of HCl x volume of solution =0.1 x (50 / 1000) =0.005mol (Mg is in excess) Number mole of Mg reacted = number of mole of HCl /2 =0.005 /2 =0.0025 mol Mass of Mg reacted = number of mole of Mg reacted x molar mass of Mg =0.0025 x 24.3 =0.06075g Rate of reaction of Mg=mass of Mg reacted / time required = 0.06075g /90 = 6.75e-4g/s ii) Rate of reaction of Mg= number of mole of Mg / time required =0.0025 /90 =2.78e-5 mol/s iii)Number of mole of hydrogen gas produced=0.0025mol volume of H gas = 0.0025 x 24 =0.06dm^3 =60cm^3 Time required = 60 /90 =0.667 cm^3/s
f.5 chem question again ~~
發問:
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When 0.36g of magnesium was added to 50 cm3 of 1.0M hydrochloric acid at room conditions , the magnesium reacted and disappeared in 90 secondsa) Write an equation for the reaction between and hydrochloric acidb) Give the average reaction reaction rate in (i) g of Mg reacted per second ;(ii) no. of moles of Mg... 顯示更多 When 0.36g of magnesium was added to 50 cm3 of 1.0M hydrochloric acid at room conditions , the magnesium reacted and disappeared in 90 seconds a) Write an equation for the reaction between and hydrochloric acid b) Give the average reaction reaction rate in (i) g of Mg reacted per second ; (ii) no. of moles of Mg reacted per second ; (iii) volume of hydrogen produced in cm3 per second , given 1 mole of hydrogen gas occupies a volume of 24000 cm3 at room conditions最佳解答:
a. Chemical equation: Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) b.i. Average rate = Mass / time = 0.36 / 90 = 0.004 g / s ii. No. of mole of Mg in 0.004 g = Mass / molar mass = 0.004 / 24.0 = 1.67 X 10-4 mol So, average rate = no. of mole / time = 1.67 X 10-4 / 90 = 1.85 X 10-6 mol / s iii. Mole ratio of Mg to H2 = 1 : 1 So, no. of mole of H2 produced = 1.67 X 10-4 mol So, volume of H2 produced per second = 1.67 X 10-4 X 24 000 = 4 cm3 / s
其他解答:
a) Mg+2HCl>MgCl2+H2 bi)Molar mass of Mg=24.3g/mol Molar mass of HCl=1.0+35.5=36.5g/mol Number of mole of Mg=mass of Mg / molar mass of Mg =0.36 / 24.3 =0.0148mol Number of mole of HCl= molarity of HCl x volume of solution =0.1 x (50 / 1000) =0.005mol (Mg is in excess) Number mole of Mg reacted = number of mole of HCl /2 =0.005 /2 =0.0025 mol Mass of Mg reacted = number of mole of Mg reacted x molar mass of Mg =0.0025 x 24.3 =0.06075g Rate of reaction of Mg=mass of Mg reacted / time required = 0.06075g /90 = 6.75e-4g/s ii) Rate of reaction of Mg= number of mole of Mg / time required =0.0025 /90 =2.78e-5 mol/s iii)Number of mole of hydrogen gas produced=0.0025mol volume of H gas = 0.0025 x 24 =0.06dm^3 =60cm^3 Time required = 60 /90 =0.667 cm^3/s
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